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(Gate 2001)
1. A reasonably general expression for
vapour liquid phase equilibrium a low
modern pressure is 0
i i i i iy P x f where is a vapour
fugacity coefficient i is the liquid activity
coefficient , and o
if is the fugacity of pure
component i. the KI value i i iy K x is
therefore, in general , a function of
(a) temperature only
(b) temperature and pressure only
(c) temperature, pressure liquid
composition xi only
(d) temperature , pressure liquid
composition xi and vapour composition
yi
2. High pressure steam is expanded
adiabatically and reversibly through a well
insulated turbine which produces some
shaft work. If the enthalpy change and
entropy change across the turbine are
represented by H and S . Respectively
for this process:
(a) H 0 & S 0
(b) H 0 & S 0
(c) H 0 & S 0
(d) H 0 & S 0
3. The maxwell relation derived form the
differential expression for the helmohtz free
energy (dA) is
(a) s v
T T
V S
(b) T v
S V
P T
(c) P s
V T
S P
(d) T v
S P
V T
4. At 1000C, water and methyleyclohexane
both have vapour pressures of 1.0 atm. also
at 100 0C the latent heats of vaporization of
these compounds are 40.63 kJ/mol for
water and 31.55 kJ/mol for methyl
cyclohexane. The vapour pressure of water
at 150 0C is 0C , the vapour pressure of meth
cyclohexane would be expected to be
(a) Significantly less than 4.69 atm
(b) Nearly equal to 4.69 atm
(c) Significantly more than 4.69 atm
(d) Indeterminate due to a lack of data
CHAPTER 2
• CHEMICAL ENGINEERING THERMODYNAMICS
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5. Air enters an adiabatic compressor at
300 K. the exit temperature for a
compression ratio of 3, assuming air to be
an ideal gas p v(y C / C 7 / 5) and the
process to be reversible is
(a) 300 (3 m2/7) (b) 300 (3 m1/5)
(c) 300 (3 m3/7) (d) 300 (3 m5/7)
(Gate 2002)
6. Which of the following conditions are
satisfied at the critical point by the P-V-T
relation of a real fluid?
(a) 2
2
TT
P P0
V V
(b) 2
2
TT
P P0, 0
V V
(c) 2
2
TT
P P0, 0
V V
(d) 2
2
TT
P P0, 0
V V
7. The number of degrees of freedom for an
azeotropic mixture of ethanol and water in
vapour liquid equilibrium is
(a) 3 (b) 1
(c) 2 (d) 0
8. The partial molar enthalpy of a
component in an ideal binary gas mixture of
compositional temperature T and pressure
P, is a function only of
(a) T (b) T and P
(c) T, P and Z (d) T and Z
9. Which of the following identities can be
most easily used to verify steam table data
for superheated steam?
(a) S V
T / V P / S
(b) S P
T / P V / S
(c) V T
P / T S/ V
(d) P T
V / T S/ P
10. Steam undergoes isentropic expansion
in a turbine form 5000 kPa and 400 0C
(entropy = 6.65 kJ/kg K) to 150 k Pa
(entropy of saturated liquid = 1.4336 kJ/kg
K, entropy of saturated vapour = 7.2234
kJ/kg K). The eixt condition of steam is
(a) superheatedvpaour
(b) partially condensed vapour with quality
of 0.9
(c) saturatedvapour
(d) partially condensed vapour with quality
of 0.1
11. A rigid vessel, containing three moles of
nitrogen gas at 30 0C, is heated to 250 0C .
assume the average heat capacities of
nitrogen to be required, neglecting the heat
capacity of the vessel, is
0 0
p vC 29.1 J / mol C and C 20.8J / mol C. The heat
required neglecting the heat capacity of the
vessel, is
(a) 13728 J (b) 19206 J
(c) 4576 J (d) 12712 J
12. 1 m3 of an ideal gas at 500 K and 1000
kPa expands reversibly to 5 times its
intialvolume in an insulated container. If
the specific heat capacity (at constant
pressue) of the gas is 21J/mol
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(a) 35 K (b) 174 K
(c) 274 K (d) 154 K
(Gate 2003)
13. for organic estimation of heat capacity
of a solid compound, one can use
(a) clapeyron’s equation
(b) gibb’s equation
(c) kopp’s rule
(d) Troution’s rule
14. One mole of nitrogen at 8 bar and 600 K
is contained is a piston cylinder
arrangement. It is brought to 1 bar
isothermally against a resisting pressure of 1
bar. The work done (in joules) by the gas is
(a) 30554 (b) 10373
(c) 4988.4 (d) 4364.9
15. For water at 3000C , it has a vapour
pressure 8592.7 kPa and fugacity 6738.9
kPa under these conditions, one mole of
water in liquid phase has a volume 25.28
cm3 and that in vapour phase 391.1 cm3.
Fugacity of water (in kPa at 9000 kpa will
be
(a) 673.89 (b) 6753.5
(c) 7058.3 (d) 90000
16. Heat capacity of air can be
approximately expressed as
CP = 26.693 + 7.365 x 10-3 T
Where Cp is J/ (mol) (K) and T is K. The
heat given off by 1 mole of air when cooled
at 1 atmospheric pressure from 500 0C to –
100 0C is
(a) 10.73 kJ (b) 16.15 kJ
(c) 18.11 kJ (d) 18.33 kJ
17. A solid metallic block weighing 5 kg has
an initial temperature of 500 0C; 40 kg of
water initially at 25 0C is contained in a
perfectly insulated tank. The metallic block
is brought into contact with water. Both of
them come to equilibrium. Specific heat of
block material is 0.4 material is 0.4 kJ kg-1K-
1. Ignoring the effect of expansion and
contraction, and also the heat capacity of
tank, the total entropy change in kJ kg-1K-1 is
(a) – 1.87 (b) 0.0
(c) 1.26 (d) 3.91
18. The following heat engine produces
power of 100,000kW. The heat engine
operates between 00 K and 300 K. it has
thermal efficiency equal to 50% of that of
the Carnot engine for the same temperature.
The rate at which heat is absorbed from the
hot reservoir is
(a) 100,000 kW
(b) 160,000 kW
(c) 200,000 kW
(d) 320,000 kW
19. At 600C, vapour pressures of methanol
and water are 84.562 kPa and 19.953 kPa
respectively an aqueous solution of
methanol at 600C exerts a pressure of
39.223 kPa; the liquid phase andvapour
phase mole fractions of methanol are 0.1686
and 0.5714 respectively. Activity coefficient
of methanol is
(a) 1.572 (b) 1.9398
(c) 3.389 (d) 4.238
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20-21 are based on the data supplied
in the paragraph below
One kg of saturated steam at 1000C and
1.01325 bar is contained in a rigid walled
vessel. It has a volume 1.673 m3. It cools to
980C; the saturation pressure is 0.943 bar;
one of water vapour under these conditions
has a volume of 1.789 m-3
20. The amount of water vapour condensed
(in kg) is
(a) 0.0 (b) 0.065
(c) 0.1 (d) 1.0
21. The latent heat of condensation (kJ kg-1)
under these conditions is
(a) 40732 (b) 2676
(c) 2263 (d) 540
(Gate 2004)
22. For an ideal gas mixture undergoing
a reversible gaseous phase chemical
reaction, the equilibrium constant
(A) Independent of pressure
(B) Increases with pressure
(C) Decreases with pressure
(D) Increases / decreases with pressure
depending on the stoichiometric
coefficients of the reaction.
23. As pressure approaches zero, the
ratio of fugacity to pressure (f/P) for a gas
approaches
(A) Zero (B) Unity
(C) Infinity (D) An indeterminate
value
24. A perfectly insulated container of
volume V is divided into two equal halves by
a partition. One side is under vacuum while
the other side has one mole of an ideal gas
(with constant heat capacity) at 298 K. If
the partition is broken, the final
temperature of the gas in the container
(A) Will be greater than 298 K
(B) Will be 298 K
(C) Will be less than 298 K
(D) Can’t be determined
25. The number of degrees of freedom
for an azeotropic mixture in a two
component vapor – liquid equilibria is / are
(A) Zero (B) One
(C) Two (D) Three
26. A car tier of volume 0.057 m3 is
inflated to 300 kPa at 300 K. After the car
is driven for ten hours, the pressure in the
tier increases to 330 kPa. Assume air is an
ideal gas and Cv for air is 21 J/(mol K). The
change in the internal energy of air in the
tier in J/mol is
(A) 380 (B) 630
(C) 760 (D) 880
27. A gas obeys P (V-b) = RT. The work
obtained from reversible isothermal
expansion of one mole of this gas from an
initial molar volume vi to a final molar
volume vf is
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(A)
f
i
VRTln
V (B)
f
i
V bRTln
V
(C)
f
i
VRTln
V b (D
f
i
V bRTln
V b
28. A cyclic engine exchanges heat with
two reservoirs maintained at 100 and
3000C, respectively. The maximum work (in
J) that can be obtained from 1000 J of heat
extracted from the hot reservoir is
(A) 349 (B) 651
(C) 667 (D) 1000
29. The vapor pressure of water is given
by sat 5000lnP A
T where A is a constant, Psat is
vapor pressure in atm, and T is temperature
in K. The vapor pressure of water in atm at
50 0C is approximately
(A) 0.07 (B) 0.09
(C) 0.11 (D) 0.13
30. At standard conditions,
N2 + 2O2 2NO2 ∆G0 = 100 kJ/mol
NO + ½ O2 NO2 ∆G0 = – 35 kJ/mol
The standard free energy of formation of
NO in kJ/mol is
(A) 15 (B) 30
(C) 85 (D) 170
(Gate 2005)
31. In van der Waals equation of state,
what are the criteria applied at the critical
point in determine the parameters ‘a’ and
‘b’?
(A) 2
20 0
T T
P P;
V V
(B) 2
20 0
T T
V V;
P P
(C) 2
20 0
V V
P P;
T T
(D) 2
20 0
P P
V V;
V T
32. Which one of the following
statements in TRUE?
(A) Heat can be fully converted into work
(B) Work cannot be fully converted into heat
(C) The efficiency of a heat engine increases
as the temperature of the heat source is
increased while keeping the
temperature of the heat sink fixed.
(D) A cyclic process can be devised whose
sole effect is to transfer heat from a lower
temperature to a higher temperature.
33. A Carnot heat engine cycle is
working with an ideal gas. The work
performed by the gas during the adiabatic
expansion and compression steps, W1 and
W2 respectively, are related as
(A) | W1 | > | W2 | (B) | W1 | < |W2 |
(C) W1 = W2 (D) W1 = – W2
34. The Van-Laar activity coefficient
model for a binary mixture is given by the
form
*
1 *
1
*
2
Aln
xA1
xB
*
2 *
2*
1
ln
1
B
xB
A x
Given γ1 = 1.40, γ2 = 1.25, x1 = 0.25, x2 =
0.75, determine the constants A* and B*,
(A) A* = 0.5, B* = 0.3
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(B) A* = 3, B* = 0.5
(C) A* = 0.333, B* = 0.2
(D) A* = 2, B* = 0.333
35. What is the actual power required to
drive a reciprocating air compressor which
has to compress 34 m3 of air per minute
from 1.013 x 105 N/m2 to 4.052 x 105 N/m2?
Assume that PV1.25 is constant, where P is
the pressure and V is the volume, and the
efficiency of the compressor is 85%.
(A) 107.9 kW (B) 200 kW
(C) 82.6 kW (D) 91.7 kW
Linked Answer Questions: 36 and 37
A frictionless cylinder piston assembly
contains an ideal gas. Initially pressure (P1)
= 100 kPa, temperature (T1) = 500 K and
volume (V1) = 700 x 10-6 m3. This system is
supplied with 100 J of heat and pressure is
maintained constant at 100 kPa. The
enthalpy variation is given by H (J/mol) =
30000 + 50 T; where T is the temperature
in K, and the universal gas constant R =
8.314 J/(mole K).
36. The final volume of the gas (V2) in m3 is
(A) 700 x 10-6
(B) 866.32 x 10-6
(C) 934.29 x 10-6
(D) 1000.23x10-6
37. The change in I.E. of the gas in J is
(A) 0 (B) 10
(C) 23.43 (D) 83.37
(Gate 2006)
38. At a given temperature and pressure, a
liquid mixture of benzene and toluene is in
equilibrium with its vapor. The available
degree(s) of freedom is (are)
(A) 0 (B) 1
(C) 2 (D) 3
39. A heat engine operates at 75% of the
maximum possible efficiency. The ratio of
the heat source temperature (in K) to the
heat sink temperature (in K) is 5/3. The
fraction of the heat supplied that is
converted to work is
(A) 0.2 (B) 0.3
(C) 0.4 (D) 0.6
40. For the isentropic expansion of an ideal
gas from the initial conditions T1, T1 to the
final conditions T2, T2, which ONE of the
following relations is valid? (γ = Cp / Cv)
(A) 1 2
2 1
P T
P T
(B) 1
1 2
2 1
P T
P T
(C) 1 1
2 2
P T
P T
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(D) 1
1 1
2 2
P T
P T
41. Match the following:
(a) Heat (i) State Function
(b) Internal energy (ii) Path Function
(c) Work
(d) Entropy
(A) (a)-(ii); (b)-(i); (c)-(i); (d)-(i)
(B) (a)-(ii); (b)-(i); (c)-(ii); (d)-(ii)
(C) (a)-(ii); (b)-(ii); (c)-(i); (d)-(i)
(D) (a)-(ii); (b)-(i); (c)-(ii); (d)-(i)
42. For a binary mixture of A and B at
400 K and 1 atm, which ONE of the
following equilibrium states deviates
significantly from ideality?
Given: 2758
6 2 sat
Aln P .T
where,
PAsat = vapor pressure of A, atm;
T = temperature, K
PA = partial pressure of A, atm,
xA = mole fraction of A in liquid; yA =
mole fraction of A in vapor
(A) xA = 0.5; yA = 0.25
(B) xA = 0.5; PA = 0.25
(C) xA = 0.5; PA = 0.5
(D) xA = 0.6; yA = 0.3
43. The molar density of water vapor at the
normal boiling point of water is 33 mol/m3.
The compressibility factor under these
conditions is close to which ONE of the
following? R = 8.314 J/(mol K)
(A) 0.75 (B) 1
(C) 1.25 (D) 1.5
(Gate 2007)
44. If TA and TB are the boiling points of
pure A and pure B respectively and TAB is
that of a non-homogeneous immiscible
mixture of A and B, then
(A) TAB < TA& TB (B) TAB > TA& TB
(C) TA> TAB > TB (D) TB> TAB > TA
45. The state of an ideal gas is changed
from (T1, P1) to T2, P2) in a constant volume
process. To calculate the change in enthalpy
Δh, ALL of the following
properties/variables are required.
(A) CV , P1 , P2
(B) CP , T1 , T2
(C) CP , T1 , T2 , P1 , P2
(D) CV , P1 , P2 , T1 , T2
46. The change in entropy of the
system, ΔSsys, undergoing a cyclic
irreversible process is
(A) Greater than 0
(B) Equal to zero
(C) Less than zero
(D) Equal to the ΔSsurroundings
47. Parameters ‘a’ and ‘b’ in the van der
Waals and other cubic equations of state
represent
(A) a – molecular weight
b – molecular polarity
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(B) a – molecular size
b – molecular attraction
(C) a – molecular size
b – molecular speed
(D) a – molecular attraction
b – molecular size
48. If R
i
E
iii mmmm ,,, are molar, partial
molar, residual and excess properties
respectively for a pure species “i”, the
mixture property M of a binary non-ideal
mixture of components 1 and 2, is given by
(A) x1 1m + x2 2m
(B) x1 m1R + x2 m2
R
(C) x1 m1 + x2 m2
(D) x1 m1E + x2 m2
E
49. For the two paths as shown in the
figure, one reversible and one irreversible,
to change the state of the system from a to b,
is
(A) ΔU, Q, W are same
(B) ΔU, is same
(C) Q, W are same
(D) ΔU, Q, are different.
50. For a pure substance, the Maxwell’s
relation obtained from the fundamental
property relation du = Tdz – Pdv is
(A) vs s
P
v
T
(B) Tv v
s
T
P
(C) Ps s
v
P
T
(D) Tv P
s
T
v
51. Which of the following represents the
Carnot cycle (ideal engine)?
52. 2 kg of steam in a piston-cylinder device
at 400 kPa and 175 °C undergoes a
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mechanically reversible, isothermal
compression to a final pressure such that
the steam becomes just saturated. What is
the work, W, required for the process?
Data:
T = 175°C, P = 400 kPa – v = 0.503 m3/kg, u
= 2606 kJ/kg, s = 7.055 kJ/kg-K
T = 175°C, satd. vapor – v = 0.216 m3/kg, u
= 2579 kJ/kg, s = 6.622 kJ/kg-K
(A) 0 kJ (B) 230 kJ
(C) 334 kJ (D) 388 kJ
53. Vapor phase hydration of C2H4 to
ethanol by the following reaction
C2H4 (g) + H2O (g) ↔ C2H5 OH (g)
Attains equilibrium at 400 K and 3 bar. The
standard Gibbs free energy change of
reaction at these conditions is Δg° = 4000
J/mol. For 2 moles of an equimolar feed of
ethylene and steam, the equation in terms of
the extent of reaction ε (in mols) at
equilibrium is
(A)
2
(2 )0.3 0
(1 )
(B)
2(1 )0.9 0
(2 )
(C)
2
0.3 0(1 )
(D)
2
(2 )0.9 0
(1 )
Linked Answer Questions 54 & 55:
A methanol-water vapor liquid system is at
equilibrium at 60°C and 60 kPa. The mole
fraction of methanol in liquid is 0.5 and in
vapor is 0.8. Vapor pressure of methanol
and water at 60°C are 85 kPa and 20 kPa
respectively. Assuming vapor phase to be
an ideal gas mixture
54. What is the activity coefficient of water
in the liquid phase?
(A) 0.3 (B) 1.2
(C) 1.6 (D) 7.5
55. What is the excess Gibbs free energy
(gE, in J/mol) of the liquid mixture?
(A) 9.7 (B) 388
(C) 422 (D) 3227
Linked Answer Questions 56 & 57:
56. A perfectly insulated cylinder of
volume 0.6 m3 is initially divided into two
parts by a thin, frictionless piston, as shown
in the figure. The smaller part of volume
0.2 m3 has ideal gas at 6 bar pressure and
100°C. The other part is evacuated.
vacuum0.2 m3
stopper
At certain instant of time t, the stopper is
removed and the piston moves out freely to
the other end. The final temperature is
(A) –140 °C (B) –33 °C
(C) 33°C (D) 100°C
57. The cylinder insulation is now
removed and the piston is pushed back to
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restore the system to its initial state. If this
is to be achieved only by doing work on the
system (no heat addition, only heat removal
allowed), what is the minimum work
required?
(A) 3.4 kJ (B) 107 kJ
(C) 132 kJ (D) 240 kJ
(Gate 2008)
58.For a Carnot refrigerator operating
between 40°C and 25°C, the coefficient of
performance is
(A) 1 (B) 1.67
(C) 19.88 (D) 39.74
59. The work done by one mole of a van
der Waals fluid undergoing reversible
isothermal expansion from initial volume Vi
to final volume Vf is
(A)
i
f
V
VRT ln
(B) lnf
i
V bRT
V b
(C) 1 1
lnf
i f i
V bRT a
V b V V
(D) 1 1
lnf
i f i
V bRT a
V b V V
60. The molar volume (v) of a binary
mixture, of species 1 and 2 having mole
fractions x1 and x2 respectively is given by
v = 220 x1 + 180 x2 + x1 x2 (90 x1 + 50 x2).
The partial molar volume of species 2 at x2 =
0.3 is
(A) 183.06 (B) 212.34
(C) 229.54 (D) 256.26
61. The standard Gibbs free energy
change and enthalpy change at 25°C for the
liquid phase reaction CH3COOH (1) +
C2H5OH (1) CH2COOC2H5(1) + H2O (1) are
given as ΔG°298 = - 4650 J/mol and ΔH°298 = -
3640 J/mol. If the solution is ideal and
enthalpy change is assumed to be constant,
the equilibrium constant at 95°C is
(A) 0.65 (B) 4.94
(C) 6.54 (D) 8.65
Linked Answer Questions 62 and 63:
A binary mixture containing species 1 and 2
forms an azeotropic at 105.4°C and 1.013
bar. The liquid phase mole fraction of
component 1 (x1) of this azeotropic is 0.62.
At 105.4°C, the pure component vapor
pressures for species 1 and 2 are 0.878 bar
and 0.665 bar, respectively. Assume that
the vapor phase is an ideal gas mixture. The
van – Laar constants, A and B, are given by
the expressions:
62. The activity coefficients ( γ1, γ2 )
under these conditions are
(A) (0.88, 0.66) (B) (1.15, 1.52),
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(C) (1.52, 1.15) (D) (1.52, 0.88)
63. The Van Laar constants (A, B) are
(A) (0.92, 0.87) (B) (1.00, 1.21),
(C) (1.12, 1.00) (D) (1.52, 1.15)
(Gate 2009)
64. An ideal gas at temperature T1 and
pressure P1 is compressed isothermally to
pressure P2 (> P1) in a closed system. Which
ONE of the following is TRUE for internal
energy (U) and Gibbs free energy (G) of the
gas at the two states?
(A) U1 = U2, G1> G2
(B) U1 = U2, G1< G2
(C) U1> U2, G1 = G2
(D) U1< U2, G1 = G2
65. For a binary mixture at constant
temperature and pressure, which ONE of
the following relations between activity
coefficient (γi) and mole fraction (xi) is
thermodynamically consistent?
(A) 2
111 21ln xx , 2
122
1ln x
(B) 2
111 21ln xx , 2
12ln x
(C)2
111 21ln xx , 2
122
1ln x
(D) 2
111 21ln xx , 2
12ln x
Common Data Questions66 and 67:
An ideal gas with molar heat capacity
5
2pC R (where R = 8.314 J / mol.K) is
compressed adiabatically from 1 bar and
300 K to pressure P2 in a closed system. The
final temperature after compression is 600
K and the mechanical efficiency of
compression is 50%.
66. The work required for compression
(in kJ/mol) is
(A) 3.74 (B) 6.24
(C) 7.48 (D) 12.48
67. The final pressure P2 (in bar) is
(A) 23/4 (B) 25/4
(C) 23/2 (D) 25/2
(Gate 2010)
68. An equi-molar liquid mixture of
species 1 and 2 is in equilibrium with its
vapor at 400 K. At this temperature, the
vapor pressures of the species are = 180 kPa
and = 120 kPa. Assuming that Raoult’s law
is valid, the value of y1 is
(A) 0.30 (B) 0.41
(C) 0.50 (D) 0.60
69. A new linear temperature scale,
denoted by °S, has been developed,
where the freezing point of water is 200°S
and the boiling point is 400°S. On this
scale, 500°S corresponds, in degrees
Celsius, to
(A) 100°C (B) 125°C
(C) 150°C (D) 300°C
70. A saturated liquid at 1500 kPa and
500 K, with an enthalpy of 750 kJ / kg, is
throttled to a liquid – vapor mixture at 150
kPa and 300 K. At the exit conditions, the
enthalpy of the saturated liquid is 500 kJ /
kg and the enthalpy of the saturated vapor is
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2500 kJ/kg. The percentage of the original
liquid, which vaporizes, is
(A) 87.5 % (B) 67%
(C) 12.5% (D) 10%
71. At constant T and P, the molar
density of a binary mixture is given by ρ = 1
+ x2, where x2 is the mole fraction of
component-2. The partial molar volume at
infinite dilution for component-1, is
(A) 0.75 (B) 1.0
(C) 2.0 (D) 4.0
(Gate 2011)
72. Minimum work (W) required
separating a binary gas mixture at a
temperature T0 and pressure P0 is,
1 2
0 1 2
21
ˆ ˆf fW RT y ln y ln
f f
where y1 and y2 are mole fractions. fpure,1 and
fpure,2 are fugacity of pure species at T0 and
P0 and f1 and f2 are fugacity of species in the
mixture at T0 , P0 and y1.
If the mixture is ideal then W is
(A) 0
(B) – RT0 [y1ln y1 + y2ln y2]
(C) RT0 [y1ln y1 + y2lny2 ]
(D) RT0
73. The partial molar enthalpies of
mixing (in J / mol) for benzene (component
1) and cyclo-hexane (component 2) at 300 K
and 1 bar are given by and, where x1 and x2
are the mole fractions. When ONE mole of
benzene is added to TWO moles of cyclo-
hexane, the enthalpy change (in J) is
(A) 3600 (B) 2400
(C) 2000 (D) 800
74. One mole of methane is contained in
a leak proof piston – cylinder assembly at 8
bar and 1000 K. The gas undergoes
isothermal expansion to 4 bar under
reversible conditions. Methane can be
considered as an ideal gas under these
conditions. The value of universal gas
constant is 8.314 J.mol–1 K–1. The heat
transferred (in kJ) during the process is
(A) 11.52 (B) 5.76
(C) 4.15 (D) 2.38
75. Two systems are available for
compressing 6 m3 / hr of ambient air to 10
bar. The first one uses a single stage
compressor (K1) and the second one uses a
multistage compressor with inter – stage
cooling (K2). Which ONE of the following
statements is INCORRECT?
(A) K2 will have knockout pots in between
the stages
(B) Discharge temperature of K1 will be
higher than that of K2
(C) K2 will consume more power than K1
(D) Cost of K2 will be more than that of K1
76. Consider a binary mixture of methyl
ethyl ketone (component 1) and toluene
(component 2). At 323 K the activity
coefficients γ1 and γ2 are given by
2
1 2 1 2 2 1ln x 4 x ,
1
2
2 1 2 2 2ln x 4 x Where x1 and x2 are
the mole fractions in the liquid mixture, and
Ψ1 and Ψ2 are parameters independent of
composition. At the same temperature, the
infinite dilution activity coefficients, and are
given by 1
ln 0.4 and
ln 0.2 . The vapor
GATE Previous Years Solved Papers The Gate Coach
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pressure of methyl ethyl ketone and toluene
at 323 K are 36.9 and 12.3 kPa respectively.
Assuming that the vapor phase is ideal, the
equilibrium pressure (in kPa) of a liquid
mixture containing 90 mol % toluene is
(A) 19 (B) 18
(C) 16 (D) 15
(Gate 2012)
77. In a throttling process, the pressure of
an ideal gas reduces by 50 % if P vC and C are
the heat capacities at constant pressure and
constant volume, respectively P VC / C ,
the specific volume will change by a factor of
(A) 2 (B) 12 /
(C) 12
/
(D) 0.5
78. If the temperature of saturated water
is increased infinitesimally at constant
entropy the resulting state of water will be
(A) Liquid
(B) Liquid- vapor coexistence
(C) Saturated vapor
(D) Solid
79. In a parallel flow heat operating
under steady state hot liquid enters at a
temperature h.inT and leaves at a
temperature h,out.T liquid enters at a
temperature c,inT and leaves at a
temperature c,outT Neglect any heat loss from
the heat exchanger to the surrounding id
h,in C,inT T then for a given time interval,
which ONE of the following statements is
true?
(A) Entropy gained by the cold stream is
GREATER than entropy lost by the hot
stream
(B) Entropy gained by the cold stream is
EQUAL to the entropy lost by the hot
stream
(C) Entropy gained by the cold stream is
LESS than the entropy lost by the hot
stream
(D) Entropy gained by the cod stream is
ZERO
80. For an exothermic irreversible
reaction which one of the following correctly
describes the dependence of the equilibrium
constant (K) with temperature (T) and
pressure (p)?
(A) K is independent of T and P
(B) K increase with an increase in T and P
(C) K increases with T and decreases with
P
(D) K decreases with an increase in T and is
independent of P
81. An insulated, evacuated container is
connected to a supply line of an ideal gas at
pressure s,P temperature sT and specific
volume sv . The container is filled with the
gas until the pressure in the container
reaches sP there is no heat transfer between
the supply line to the container, and kinetic
and potential energies are negligible. If
1PC and C are the heat capacities at constant
pressure and constant volume respectively
P vC / C , then the final temperature of
gas in the container is
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(A) sT (B)
sT
(C) sI T
(D) 1 sT /
82. Consider a binary liquid mixture at
constant temperature T and pressure P. if
the enthalpy change of mixing
1 2 1 25 H x x , where x and x are the mole
fraction of species 1 and 2 respectively and
the entropy change of mixing
1 2 2 S x In +x In x (with R = 8.314 J /
mol.K) then the minimum value of the
Gibbs free energy change of mixing at 300 K
occurs when
(A) 1
0x
(B) 1
0 2x .
(C) 1
0 4x .
(D) 1
0 5x .
(GATE 2013)
83. A gaseous system contains H2, I2,
and HI, which participate in the gas-phase
reaction
2HI H2 + I2
At a state of reaction equilibrium, the
number of thermodynamic degrees of
freedom is_______
84. The thermodynamic state of a closed
system containing a pure fluid changes from
(T1, p1) to (T2, p2), where T and p denote the
temperature and pressure, respectively. Let
Q denote the heat absorbed (> 0 if absorbed
by the system) and W the work done (> 0 if
done by the system). Neglect changes in
kinetic and potential energies. Which one of
the following is CORRECT?
(A) Q is path-independent and W is path-
dependent
(B) Q is path-dependent and W is path-
independent
(C) (Q − W) is path-independent
(D) (Q+W) is path-independent
85. An equation of state is explicit in
pressure p and cubic in the specific volume
v. At the critical point ‘c’, the isotherm
passing through ‘c’ satisfies
(A) 0,02
2
v
p
v
p
(B) 0,02
2
v
p
v
p
(C) 0,02
2
v
p
v
p
(D) 0,02
2
v
p
v
p
86. The units of the isothermal
compressibility are
(A) 3m (B)
1Pa
(C) 13 Pam (D)
13 Pam
87. In a process occurring in a closed
system F, the heat transferred from F to the
surroundings E is 600 J. If the temperature
of E is 300 K and that of F is in the range
380 – 400 K, the entropy changes of the
surroundings (∆SE) and system (∆SF), in
J/K, are given by
(A) 2,2 FE SS
(B) 2,2 FE SS
(C) 2,2 FE SS
(D) 2,2 FE SS
88. A binary liquid mixture is in
equilibrium with its vapor at a temperature
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T = 300 K. The liquid mole fraction x1 of
species 1 is 0.4 and the molar excess Gibbs
free energy is 200 J/mol. The value of the
universal gas constant is 8.314 J/mol-K, and
i γ denotes the liquid-phase activity
coefficient of species i. If ln (γ1) = 0.09, then
the value of ln(γ2), up to 2 digits after the
decimal point, is
(Gate 2014)
89. From the following list, identify the
properties which are equal in both vapour
and liquid phases at equilibrium
P. Density
Q. Temperature
R. Chemical potential
S. Enthalpy
(A) P and Q only (B) Q and R only
(C) R and S only (D) P and S only
90. In a closed system, the isentropic
expansion of an ideal gas with constant
specific heats is represented by
91. Match the following
Group 1 Group 2
(P)
ijnPTin
G
,,
I. Arrhenius
equation
(Q)
ijnVSin
G
,,
II. Reaction
Equilibrium
constant
(R)
RT
Greaction
0
exp III. Chemical
Potential
(S) 0, PTiidn IV. Gibbs –
Duhem equation
(A) Q-III, R-I, S-II
(B) Q-III, R-II, S-IV
(C) P-III, R-II, S-IV
(D) P-III, R-IV, S-I
92. Which ONE of the following is
CORRECT for an ideal gas in a closed
system?
(A) VS S
UnRV
V
U
(B) PS S
HnRP
P
H
(C) PS S
HnRV
V
U
(D) VS S
UnRP
P
H
93. Consider a binary liquid mixture at
equilibrium with its vapour at 250 C
Antoine equation for this system is given as
log10pisat A -
B
t c where t is in 0C and P in
Torr.
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The Antoine constant (A, B, and C) for the
system are guven in the following table
Component A B C
1 7.0 1210 230
2 6.5 1206 223
The vapor phase is assumed to be ideal and
the activity coefficients (γi) for the non ideal
liquid phjase are given by
In (γ1) = x22[ 2-0.6 x1]
In (γ2) = x12 [1.7 + 0.6x2]
If the mole fraction of component 1 in liquid
phase (x1) is 0.1 then the mole fraction of
component 1 in vapor phase (y1) is ………
(Gate 2015)
94. If v, u, s and g represent respectively
the molar volume, molar internal energy,
molar entropy and molar Gibbs free energy,
then match the entries in the left and right
columns below and choose the correct
option.
(P) S
u
v
(I) Temperature
(Q) T
g
P
(II) Pressure
(R) P
g
T
(III) V
(S) V
u
s
(IV) S
(A) P - II, Q - III, R - IV, S - I
(B) P - II, Q - IV, R - III, S - I
(C) P - I, Q - IV, R - II, S - III
(D) P - III, Q - II, R - IV, S - I
95. For a gas phase cracking reaction A
→B + C at 300OC, the Gibbs free energy of
the reaction at this temperature is
2750 /OG J mol . The pressure is 1 bar
and the gas phase can be assumed to be
ideal. The universal gas constant R =
8.314J/mol. K. The fractional molar
conversion of A at equilibrium is:
(A) 0.44 (B) 0.50
(C) 0.64 (D) 0.80
96. For a pure liquid, the rate of change
of vapour pressure with temperature is 0.1
bar/K in the temperature range of 300 to
350 K. if the boiling point of the liquid at 2
bar is 320 K, the temperature (in K) at
which it will boil at 1 bar (up to one decimal
place) is ______
97. Three identical closed systems of a
pure gas are taken from an initial
temperature and pressure (T1, P1) to a final
state (T2, P2), each by a different path.
Which of the following in Always true for
the three systems? (∆ represents the change
between the initial and final states: U, S, G,
Q and W are internal energy, entropy, Gibbs
free energy, heat added and work done,
respectively.)
(A) ∆U, ∆S, Q are same
(B) W, ∆U, ∆G are same
(C) ∆S, W, Q are same
(D) ∆G, ∆U, ∆S are same
98. Which of the following can change if
only the catalyst is changed for a reaction
system?
(A) Enthalpy of reaction
(B) Activation energy
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(C) Free energy of the reaction
(D) Equilibrium constant
99. An ideal gas is initially at a pressure
of 0.1 MPa and a total volume of 2m3. It is
first compressed to 1MPa by a reversible
adiabatic process and then cooled at
constant pressure to a final volume of
0.2m3. The total work done (in kJ) on the
gas for the entire process (up to one decimal
place) is ______
Data: R = 8.314 J/mol-K; heat capacity at
constant pressure (CP) = 2.5R
100. Given that molar residual Gibbs free
energy, gR, and molar residual volume VR,
are related as
R RPg v
dP,RT RT0
Find gR at T = 27 0C and P = 0.2MPa. The
gas may be assumed to follow the viral
equation of state, Z = 1+BP/RT, where B= -
10 – 4 m3/mol at the given conditions
(R = 8.314 J/mol-K). The value of gR in
J/mol is:
(A) 0.08 (B) −2.4
(C) 20 (D) −20
101. A binary mixture of components (1)
and (2) forms an azeotrope at 1300C and x1
= 0.3. the liquid phase non-ideality is
described by In 21 1 22
Ax and In , are the
activity coefficient and x1 , x2 are the liquid
phase mole fractions. For both
components, the fugacity coefficients are
0.9 at the isotropic composition. Saturated
vapor pressures are at 1300C are P1sat = 70
bar, P2sat= 30 bar
The total pressure in bars for the above
azeotropic system (up to two decimal
places) is
(Gate 2016)
102. The partial molar enthalpy (in
kJ/mol) of species 1 in a binary mixture is
given by2
21
2
21 100602 xxxh , where
21 and xx are the mole fractions of species 1
and 2, respectively. The partial molar
enthalpy (in kJ/mol, rounded off to the first
decimal place) of species 1 at infinite
dilution is ________
103. A binary liquid mixture of benzene
and toluene contains 20 mol% of benzene.
At 350 K the vapour pressures of pure
benzene and pure toluene are 92 kPa and 35
kPa, respectively. The mixture follows
Raoult’s law. The equilibrium vapour phase
mole fraction (rounded off to the second
decimal place) of benzene in contact with
this liquid mixture at 350 K is _____
104. An ideal gas is adiabatically and
irreversibly compressed from 3 bar and 300
K to 6 bar in a closed system. The work
required for the irreversible compression is
1.5 times the work that is required for
reversible compression from the same
initial temperature and pressure to the same
final pressure. The molar heat capacity of
the gas at constant volume is 30 J mol‒1 K‒1
(assumed to be independent of
temperature); universal gas constant, R is
8.314 J mol‒1 K‒1; ratio of molar heat
capacities is 1.277. The temperature (in K,
rounded off to the first decimal place) of the
gas at the final state in the irreversible
compression case is _______
105. A gas obeying the Clausius equation
of state is isothermally compressed from 5
MPa to 15 MPa in a closed system at 400 K.
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The Clausius equation of state is
)(Tbv
RTP
where P is the pressure, T is
the temperature, v is the molar volume and
R is the universal gas constant. The
parameter b in the above equation varies
with temperature as TbbTb 10)( with 0b
= 4 × 10‒5 m3mol‒1 and 1b = 1.35 × 10‒7
m3mol‒1K‒1. The effect of pressure on the
molar enthalpy (h) at a constant
temperature is given by
T
vTv
P
h
T
. Let hi and hf denote
the initial and final molar enthalpies,
respectively. The change in the molar
enthalpy (in J mol‒1, rounded off to the first
decimal place) for this process is ______
106. A binary system at a constant
pressure with species ‘1’ and ‘2’ is described
by the two-suffix Margules equation,
213 xxRT
gE
,where Eg is the molar excess
Gibbs free energy, R is the universal gas
constant, T is the temperature and 21 and xx
are the mole fractions of species 1 and 2,
respectively.
At a temperature T, RT
g1 = 1 and RT
g2 = 2,
where 1g and 2g are the molar Gibbs free
energies of pure species 1 and 2,
respectively. At the same temperature, g
represents the molar Gibbs free energy of
the mixture. For a binary mixture with 40
mole % of species 1, the value (rounded off
to the second decimal place) of RT
g is
(Gate 2017)
107. The volumetric properties of two
gases M and N described by the generalized
compressibility chart which expresses the
compressibility factor (Z) as a function of
reduced pressure and reduced temperature
only. The operating pressure (P) and
temperature (T) of two gases M and N
along with their critical properties (PC,Tc)
are given in the table below.
Gas P
(bar)
T (K) PC
(bar)
TC
(K)
M 25 300 75 150
N 75 1000 225 500
ZM and ZN are the compressibility factor of
the gases M and N under the given
operating conditions respectively.
The relation between ZM and ZN is
(a) 8M NZ Z (b) 3
M NZ Z
(c) M NZ Z
(d) 0 333
M NZ . Z
108. Water is heated at atmospheric
pressure from 400C to 800 C using two
different process. In process I, the heating is
done by a source at 800C. In process II, the
water is first heated form 400C to 600C by a
source at 600C, and then from 600C to 800 C
by another source at 800C. Identify the
correct statement.
(a) Enthalpy change of water in process I is
greater than enthalpy change in process II
(B) Enthalpy change of water in process II is
greater than enthalpy change in process I
(c) Process I is closer to reversibility
(d) Process II is closer to reversibility
109. The vapour pressure of a pure
substance at a temperature T is 30 bar. The
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actual and ideal gas values of g /RT for the
saturated vapour at this temperature T and
30 bar are 7.0 and 7.7 respectively. Here, g
is the molar Gibbs free energy and R is the
universal gas constant the fugacity of the
saturated liquid at these conditions,
rounded to 1 decimal place is ___bar
110. The pressure of a liquid is increased
isothermal compressibility. the molar
volume of the liquid decreases from 50.45
10-6 m3/mol to 48 10-6 m3/mol during this
process. The isothermal compressibility of
the liquid is 10-9 Pa-1, which can be assumed
to be independent of pressure The change in
the molar Gibbs free energy of the liquid,
rounded to nearest integer, is ____J/mol.
111. A sparingly soluble gas (solute) is in
equilibrium with a solvent at 10 bar. The
mole fraction of the solvent in the gas phase
is 0.01 At the operating temperature and
pressure, the fugacity coefficient of the
solute in the gas phase and the Henry’s law
constant are 0.92 and 1000 bar,
respectively. Assume that the liquid phase
obeys Henry’s law. The mole percentage of
the salute in the liquid phase rounded to 2
decimal places, is ____
(Gate 2018)
112.Under isothermal condition, a vertical
tube of length L = 100 m contains a gas of
molecular weight equal to 60. The pressure
and temperature at the top of the tube are
100 kPa and 250C respectively. Consider the
universal gas constant and acceleration due
to gravity as 8.314 J mol-1 K-1 and 9.81 m s-
2respectively. If the gas is ideal, the pressure
(in kPa) at the bottom of the tube will be
______
113. Consider the following properties: (P)
temperature (Q) specific gravity (R)
chemical potential (S) volume. The option
which lists ALL the intensive properties is
(A) P (B) P and Q
(C) P, Q, and R (D) P, Q, R and S
114. In a closed piston-cylinder system,
methane was observed to obey the following
equation of state P(V-nb) = nRT where b =
0.029 m3/mol. The temperature and volume
are 500°C and 5 m3 respectively for 100
moles of methane. At this state of the
system, the isobaric rate of change of
temperature with volume is (0C/m3) _____
(rounded off to second decimal place).
115. G denotes the Gibbs free energy of a
binary mixture, nT denotes the total number
of moles present in the system, 1 is the
chemical potential of the component
( 1 1 20 and ), ix is the mole
fraction of the component. The correct
variation ofG
nT(J/mol) at constant temperature
and pressure is given by
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Answer Key Table
1 C
2 B
3 D
4 A
5 A
6 C
7 B
8 D
9 D
10 B
11 B
12 B
13 C
14 B
15 B
16 C
17 1.249 = 1.26
18 D
19 A
20 B
21 B
22 A
23 B
24 B
25 B
26 B
27 D
28 A
29 D
30 C
31 A
32 C
33 D
34 B
35 A
36 B
37 D
38 C
39 B
40 B
41 D
42 C
43 B
44 A
45 B
46 A
47 D
48 A
49 B
50 A
51 C
52 C
53 C
54 B
55 C
56 D
57 C
58 C
59 D
60 B
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61 B
62 B
63 C
64 B
65 D
66 C
67 D
68 D
69 C
70 C
71 A
72 B
73 D
74 B
75 C
76 C
77 B
78 A
79 A
80 D
81 A
82 A
83 3
84 C
85 D
86 B
87 A
88 0.0736
89 B
90 D
91 C
92 D
93 0.693
94 A
95 D
96 310 K
97 D
98 B
99 750 kJ
100 D
101 27.54
102 -58
103 0.396
104 373 K
105 400 J /mol
106 1.64
107 C
108 D
109 14.9
110 2511.4
111 0.91
112 102.375
113 C
114 368.116
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Solutions
(Gate 2001)
1. Sol. C
0
i i i i, y P x f
ii
i
yK
x = equilibrium constant form
equation
0
i ii
i
fK
P
Where: I = liquid phase activity coefficient =
f (T, p, xi)
0
if = fugacity of pure component = f (T, p)
i = Vapopur fugacity coefficient = f (T, P)
Ki = f (T , P, xi)
2. Sol. B
Given adiabatic and reversible means
isentropic
So, S 0
sH W (shaft work) 0
3. Sol. D
Notification a – molar Helmholtz free energy
U – Molar internal energy
g – molargibbs free energy
M – Molar flow rates
a = U – Ts
da = dU – T.ds - s dT
da = (T ds – Pdv ) – T ds – s d T
da = - P dv – sdT
Now T v
a aP and s
V T
T v Tv T
a a s
T V V T V
Therefore, V T
P s
T V
“a” is a state function
T V V T
a a
T V V T
4. Sol.A
Clausius – clapeyron equation
2
1
vapvap
T
vap1 2
T
P H 1 1In
R T TP
For methyl cyclohexane
0
0
vap vap
150 MCH
vap
100
P H 1 1In
R 373 423P
For water
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0
0
vap vap
150 w
vap
100
(P ) H 1 1In
(P ) R 373 423
Divide equation 0
0
0
0
vap vap
150 MCH MCH
vap vap
w100 MCH
vap
150 W
vap
100 W
(P ) HIn
(P ) H
(P )In
(P )
Given
00
0
vap VAP vap
W100 w100 MCH
vap vap
MCH 150 W
P (p ) 1 atm H 40.63 kJ / mol
H 31.55 kJ / mol (P ) 4.69 atm
00
0
0
vap vap
150 w150 MCH
vap
150 MCH
vap
150 MCH
31.55In P In (P )
40.63
31.55In P In (4.69)
40.63
In P 3.320
5. Sol. A
For adiabatic process
1
2 2
1 1
T P
T P
Given; 2
1
P3
P
1
7T 300 K
5
So,
71
5
7 2
2 5 72
T3 T 300 3
300
(Gate 2002)
6. Sol. C
At critical point 2
2
TT
P P0
V V
Critical point is a state at which no phase
boundaries exist
7. Sol. B
Gibbs phase rule
F = C – P + 2 –r-s
Given
C = No. of component = 2 (water and ethanol)
P = No. of phase = 2 (liquid and vapour)
r =No. of independent chemical reaction=0
s = 1, for a zero tropic mixture
So, F = 2 – 2 + 2 - 0 – 1 = 1
8. Sol. (D)
9. Sol. (D)
Values of V, S, U, h are given for differential
temperature at constant pressure therefore
TP
V S
T P
Can be used easily for verify steam data for
super heated steam.
10. Sol. (b)
Isentropic means adiabatic reversible
in out
i v
S S
6.65 S x(S S )
6.65 1.4336 x(7.2234 1.4336)
x 0.90
Mixture of saturated liquid and volume
mixture with quality 0.90
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11. Sol. B
Heat required for constant volume
Q = n CP (T2 – T1)
= 3 x 29.1 x (250 – 30) = 19206 J
12. Sol. B
For adiabatic process
2 2 7 2 2 4
2 1
1 2
p P
v P
H S O ( ) H O( ) 2H SO ( )
T VSo,
T V
C C 21r 1.655
V C R 21 8.314
r 1
12 1
2
(1.655 1)
2 1
VT T
V
1500 V 5 V (given)
5
174.24 K
(Gate 2003)
13. Sol. C
Kopp’s rule Molar heat capacity of a solid of a
solid substance can be obtained by adding the
particular value for the various atoms in the
formula of the substance
H Li Be B C N O F other
10 21 15 13 8 18 20 26 J / deg mole
14. Sol. B
For isothermal process
Work done = n RT In 1
2
P
P
81 8.314 600 In 10373.08
1
+ ve sign shows work done by the system
15. Sol. B
3
3
6738 9
25 28 9000 8592 7
8314 6 573 15
6753 5
satl
sat
Vfln p p
RTf
putting values,
fln
. kPa
cm. . kPa
mol
kPa.cm. . K
mol.K
f . kPa
16. Sol. C
2
1
s
T
p
T
P
p (T,P) sat
P
ssat
H n C dT
1C 26.693 7.365F F (p) exp V dP
RT
V (P P )F
RT
6 3 3
3
25.28 10 (9000 10 8592.7 10 )6738.9 exp
8.314 573
6753.48 6753.510 T Given
for n 1
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s
2
1
P
(T,P) sat
P
Ts
sat
T6 3 3
3
1(26.693 7.365F F (p) exp V dP
RT
V (P P )F
H RT
25.28 10 (9000 10 8592.7 10 )6738.9 exp
8.314 573
6753.48 6753.510 T)dT
2 2
1 1
3T T2
T T
32 2
2 1 2 1
7.365 10H 26.693T I T I
2
7.365 10H 26.693 (T T ) T T
2
0
1
0
2
0
2
32 2
Given ;T 500 C 77 K
T 100 C 173K
T 100 C 173K
7.365 10H 26.693 (173 773) (173 773 )
2
H 18105.987 J
H 18.11 KJ
Here negative sign indicates heat is given off.
17. Sol. (c)
By energy balance
Heat given by block = heat taken by water
Block
water
P i f P f iBlock water
i
i
f f
f
mC T T mC T T
Given; T 500 273 773k;
T 25 273 298K
5 0.4 (773 T ) 40 4.18 (T 298)
T 303.61 K
total Block water
f fP Block P
i i water
S S S
T TmC In mC In
T T
303.61 303.615 0.4 In 40 4.18 In
773 298
1.869 3.118 1.249 1.26
18. Sol. D
Carnot engine efficiency
1 2c
1
T T 800 3000.625
T 800
Thermal efficiency = H c0.5
0.5 0.625 0.3125
H
work done by actual engine W0.3125
Heat absorbed by engine Q
W 100000 kW
100000Q 320000kW
0.3125
19. Sol. A
vap
1 1 1 1y p x p ; ; 1 stands for methanol
activity coefficient
11 vap
1 1
y p 0.5714 39.2231.572
x p 0.1686 84.562
20. Sol. B
Mass of water condensed + mass of water
vaporization = mass of liquid and vapor (1 lg)
Mass of water condensed = 1 – mass of water
vaporization
specific vol. of mix specific vol. of sat. liq1
specific vol. of sat. vap. spefific vol. of sat. liq
mass of liq. vapour
1.673 1 0.0011 1 0.0065 kg
1.789 0.001
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21. Sol. B
Clausius – clapeyron equation
dp
dT T V
V specific volume change
vV V
3 3
v
v
v
v
V 1.789m / kg and V 0.001 m / kg
V .V
V V
dp
dT TV
Assume satdvap. As an ideal gas
v
RTV
P
dP P
dT T RT
(Gate 2004)
22. (A)
For an ideal gas mixture undergoing a
reversible gas phase chemical reaction,
Consider a A+b B cC dD
The equilibrium constant is given by,
c d
c Dp a b
A b
P .pK
P .p
23. (B)
As the pressure approaches zero the ratio of
fugacity to pressure (f/p) for a gas
approaches.
0
1
Since as P , f p
f / p
Hence (b) is the correct answer.
24. Sol. (B)
It is a case of free expansion,
1 2 1 2
2 1 2 1
2 1
0 0
0 0
298
Q , w and
therefore u u i.e. (T T )
andT T k
Hence(B)iscorrectanswer
25. Sol. (B)
The system consists of two non-reacting
species in two phases, if there were no
zoetrope then
2 2 2 2 0 2 F N r
But is azeotropic mixer, this provides on an
additional equation i ix y
Thus we have to use equation
2
2 2 2 0 1 1
F N r S
F =
Hence (b) is the correct answer.
26. (B)
For ideal gas PV = RT
1 1300Given: p kPa, T =300K
2 2
1 1
2 2
2
2
330
300 300
330
P KPa, T =?
P TFor constant volume process,
P T
T
T
v
= 330
Change in internal energy, U = C T
= 21 (332-300) = 630 J/mol
Change in internal energy = 630 J/mol
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27. (D)
P(v b) RT
1 2
f
f
i
i
vv
vv
f
i
RTP
v b
RTw PdV dv
v b
v bRT n Hence
v b
D is the correct answer
28. Sol. (A)
Efficiency of the cycle =
2
1
3731 1 1000
573
349 04
W.D H.S
TQ
T
. J
Hence A is the correct answer
Maximum work obtained 200
1000573
349.04
Hence (A) is the correct answer,
29. Sol. (D)
Given vapor pressure relation is,
0
5000
1 100
5000
373
5000
373
5000 500
373 323
0 1255
SAT
sat
sat
sat
ln P A ,T
we know that
p atm, at T C
ln (1) =A
A =
lnP
P .
30. Sol. (C)
given that
0
2 2 2
0
2 2
0
2 2
20 2 100
135
2
2
2 2 70
N NO G kJ / mol ...(i)
NO O NO G kJ / mol ...(ii)
Multiplying equation (ii) by , we have
NO O NO G kJ / mol ... (iii)
Substracting equation (iii) from (i),w0
2 2 2
0
2
0
2 2 2
0
2 2
2 2 100
2 2 70
2 0 170
2 170
e get
N O NO ; G kJ / mol
NO O NO; G ( kJ / mol)
N O NO ; G kJ / mol
N O NO; G kJ / mol
Thus for one mole of NO, 0 85 / G kJ mol
(Gate 2005)
31. (A)
Vander Waals equation of state at the critical
point (A) Is the correct answer
32. (C)
The efficiency of a heat engine increases as
the temperature of the heat source is
increased while keeping the temperature of
the heat sink fixed. (C) is the correct answer
33. (D)
2 2 3 3
2 3 1
2 3
1
1
p v p vw w
R(T T )
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2
4 4 1 1
4 1 2
42
1
H LR(T T )b ac
p v p vw w
4 1
1
R(T T )
1
1
L H
H L
R(T T )
R(T T )
Thus w1 = – w2
Hence (D) is the correct answer
34. Sol. (B)
Putting the given values, we have
2
2
2
2
1 4 13
1 33
31
31 4 5
Aln( . ) A
B
A A ...(i)
B
Band, ln(1.25) B
A
B . B (ii)
A
Solving equations (i) and (ii), we get A=3, B=0.5
35. (A) Power required =
11
21 1
1
5
1 25
3
1
1 25 1 013 10 34 25
25 85 80 4 1
107 88 10
107 88
n
n
Comp
.
pp v
pn
n
. ( . ) .
. .
. w
. kW
(A)is thecorrectanswer
36. Sol. B)
We know that
Ideal Gas Equation of state,
1 1 1p v nRT
3 6
1 1
1
1 2 2 1 2 1
2
2
1 2
1 2
6
1 2
2
1
6
2
100 10 700 100 01684
8 314 500
50
100 0 01684 50 500
618 76
700 10 619
500
866 6 10
p vn . mol
RT .
constant pressure process,
Q n H H n (T T )
. (T )
T . K
For constant pressure,
V V
T T
V TV
T
V . 3m
37. Sol. (D)
We know that
1 2 1 2 2 1
2 1 1 2 2 1
13 16100 100 10 866 26 700 16
83 374
Q w (U U )
U U Q p(V V )
( . )
. J
(D)is thecorrectanswer
(Gate 2006)
38. Sol. (C)
F = C-P+2: Here c=2 (benzene and toluene),
P=2 (liquid and vapour). Therefore, F=2
F=C-P+2-0-0
=2-2+2-0-0=2
39. Sol . (B)
We know that
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0 75 1
30 75 1
5
0 3
LT.
T
.
w.
q
(B)is thecorrectanswer
40. (B) we know that
1 1
1 2
1 2
T T
p p
1
1
1 1
2 2
1 1
2 2
rT p
T p
T p
T p
(B)is thecorrectanswer
41. Sol. D
(a) (ii)
(b) (i)
(c) (ii)
(d) (i)
Hence (D) is the correct answer
42. (C)
given that
2758
6 2400
0 49907
0 5 0 5
.
ln .
.
( ) ,
'
o ,
. ; .
maximum
sat
A
sn
A
A A
P
P
The deviation obtained in step A is
Applying Roult s Law and applying it all
options deviation is btained
x P
43. (B) Given:
3
3
3
3
10 030
33
8 314 373 1
1 101325
0 0306
0 03001
0 0306
realgas
idealgas
mrealgas molmol
m
Jmol
idealgas
mmol
vCompressiblity Factor, Z
v
where, v specific volume m / mol
According to the problem,
v .
. KRT atmv
p atm Pa
.
.Z .
.0
(Gate 2007)
44. Sol. (A)
For an immiscible mixture, the boiling point
of the mixture is always less than the boiling
point of each individual component. (See the
concept of steam distillation of high boiling
organic compounds) (A) Is the correct
answer
45. Sol. (B)
46. Sol. (A)
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Every process proceeds in such direction that
total entropy change associated with it will be
positive. (A) is the correct answer
47. Sol. (D) is the correct answer 48. Sol. (A) is the correct answer. 49. Sol. (B) is the correct answer 50. Sol. (A) Given,
du = Tds – Pdv
This is an exact differential equation, so
vs
T P
s
(A) Is the correct answer
51. Sol. (C) is the correct answer
52. Sol. (C) We know that
1 2 2 2
2 1
1 2 1 2 2 1
1 2
1 2 1 2
448 6 622 77 055
193 9984
21579 2606 27
193 484 27 166 984
2 166 984
333 968
q T(s s ) ( . . )
. kJ / kg
u u kJ / kg
q w (u u )
kJw . .
kg
W m w ( . )
. kJ
ve sign indicates that work is reqd.
hence, C is the co
rrect answer
53. Sol. (C)
We have:
2 5
2 4 2
2 5
2
0
4000 8 314 400
0 3
0 3
1 1 1 1
2
1
2
p y
y p
C H OH
y
C H H o
p
C H OH
H O
For the given reaction
G RTln k
putting values,
J J. k ln k
mol mol.k
k .
& here we know that
K K .p
K K .p
yWhere, K
y .y
K K .
y
y
2 4
2
1
2
20 9 0
1
C Hy
on solving we get :
( ).
54. Sol. (B)
Vapor liquid equilibrium relationship is given
by
0 2 60 0 5 20
1 2
sat.
i i i i
i
i
y p x p
Hence, for water in liquid phase activity coefficient,
. .
.
55. Sol. (C)
Activity coefficient of Methanol in liquid
phase,
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1 1 2 2
8 60 85
0
i
i
E
E
0. = 5
= 1.129.
G x ln x ln RT
G = 8.314 333 .5 {ln 1.2+ln 1.129}
= 420.34
= 422 J/mol
56. Sol. (D)
it is a case of free expansion temperature
remains same i.e. 1000 C.
(D) Is the correct answer
57. Sol. (C)
Isothermal compression,
22
1 2 1 1
1
2
2 2
1
4
0 26 100 0 2
0 6
131 83
vw p v ln b ac
v
vp v ln
v
.. ln
.
. kJ
– ve sign indicates that work is reqd.
(C) Is the correct answer
(Gate 2008)
58. Sol. (C)
29819 87
313 298
L
H L
TCOP .
T T
Hence, (C) Is the correct answer
59. Sol. (D)
Real gas equation is
2
1 2 2
f f
i i
f
i
v V
v v
v
v
ap (V b) RT
V
RT aw PdV dv
V b v
aRTln(v b) a
V
1 1
f
i f i
v bRTln a
v b v v
(D)is thecorrectanswer
60. Sol. (B)
We know that
2 1
1
dV
V V xdx
1 1 1 1 1
2 1
2 3
1 1 1
220 180 1 1 40 50
1
90 10 40 180
V x ( x ) ( x )x ( x )
(x x )
V x x x
2 21
1 1 1
1
90 20 120 x dV
x x xdx
3 2
2 1 180 10 180
hence,
V x x
1 2
2
At x = 0.7 and x = 0.3
V = 212.34
61. Sol. (B)
0
2984650 G J / mol
0
298
0
3640
H J / mol
G RT lnK
G RT lnK
1
2 1 2
2
4550
8 314 298
6 274 298
1 1
6 274 3640 1 1
8 314 298 368
4 94
lnK .
K . at K
K HWe know, ln
k R T T
. ln
K .
K .
62. Sol. (B)
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Activity coefficient i
i v
i i
y P
x p
1 1
1
1
2
2
At Azeotrope y
1.013 1.15
0.878
1.013 1.52
0.665
v
v
x
p
p
p
p
63. Sol. (C)
we have
2
0 48 1 521 1 15 1 12
0 62 1 15
. ln( . )A ln( . ) .
. ln( . )
2
0 62 1 151 1 52 1 00
0 48 1 52
. ln( .B ln( . ) .
. ln( . )
(Gate 2009)
64. Sol. (B)
65. Sol. (D)
The thermodynamics consistency of activity
coefficients for a binary mixture can be
cheeked by Gibbs-Duhem equation,
1 2
1 2
1 2
2
1 1 1
1
1 1
1
1
1 1 1
1
1
1 2
0 2 2 2 1
2 1
2
dln dlnx x ( )
dx dx
for all options, ln x x
and we have to find ln :
dlnhence, x x
dx
dlnx x x
dx
1
2
2 1 1
2
2
1 1 1
1
2
1
1
2
2
2 1
1 2 1
2
from equation (1),
dlnx x x
dx
dlnor, x x x
dx
dlnx
dx
ln x
66. Sol. (C)
we have
1 1 2 2
1 2
5
2
3
2
5
3
1
1
8 314 300 600
20 5
3
7482 6
7 4826
p V
v p
p
v
Mech
Mech
C C R
C C R R R
R
C
C
p v p vW.D
(r )
R T T
(r )
. ( )
.
. J / mol
. kJ / mol
Here, –ve sign indicates that work is reqd.
67. Sol. (C)
1 2
1 1
1 2
T T
p p
2
2 2
1 1
5 3
2 3
5
2
6001
30
2
/
/
p T
p T
p
bar
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(D) Is the correct answer
(Gate 2010)
68. Sol. (D)
for Binary solution x1 + x2 = 1
For equimolar mixture, x1 = x2 = 0.5
From Raoult’s law,
sat
1 1 1
sat
2 2 2
1 2
sat sat
1 1 2 2
sat
1 1 1
sat
1 1 1
sat
1 11
1
p x p
p x p
p p p
p x p x p
0.5 180 0.5 120
p 150kpa
p x p
y p x p
x p 0.5 180y
p 150
y 0.6
69. Sol. (C)
0
C 0 S 200
100 0 400 200
S 500
C (500 200)1.5
100 (400 200)
C 150 C
70. Sol. (C)
Given:
F = 1 kg
P = 1500 kPa
T = 500 K
(1-x)kg
Hp = 750 kJ/kg,
T = 300 k, P = 150 kPa
Hc = 500 kJ/kg
Take energy balance
Input heat = vapor heat + liquid. Heat
F. HF = x Hv + (1-x) Hl
750 = x 2500 + (1-x) 500
Solve it for x
x = 0.125 =12.5%
71. Sol. (A)
2
1 1
1
V
P X
1 2
1 2
1 2
1
1
1
At infinite dilution, x x
dvV V X
dx x
2
2 2
2
1 1
2 2
1
1 1
1 1
1 1
2 2
1 11
2 2
xx x
d = x
dx x
= x ( )( x )
= 0.75
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(Gate 2011)
72. Sol. (B)
For ideal mixture.
i i
0 1 1 2 2
i
according to randall rule for an ideal gas
f y .f
putting this for two component into given equation
W RT y lny y lny
hence, (B) is the correct answer.
73. Sol. (D)
1 21 2mix
H x H x H
1 2
2
1 2
2
2 1
1 1 2 2
1 2 3 1 2 3
3600 1600
3600 400
1 21600 400 800
3 3mix
x x
H X
H x
H
74. (B)
Isothermal expansion
1
1 2 1 2
2
81 8 314 100
4
5762 8
5 762
pQ w nRTln
p
. ln
. J
. kJ
(B) is thecorrectanswer
75. Sol. (C) is the correct answer.
76. Sol. (C) given:
(Gate 2012)
77. Sol. (B)
Throttling process adiabatic process
VP constant
1 1 1
2 2 2
12
1
0 5
2 /
P V P.
P V P
V
V
78. Sol. (A)
At constant entropy, no phase change, hence
state of water is liquid
Hence A is correct answer
79. Sol. (A)
0 system surrs s
0 0M L
L H
Q Q
T T
Q Q
T T
Thus entropy change of cold fluid is
more than that of hot fluid .
Hence(A)is thecorrectanswer
80. Sol. (D)
Equilibrium constant is only being function of
temperature according to Van’t Hoff equation,
(D) is answer
81. Sol. (A)
we have
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2
2
1 2 1 1 1 2 2
1 2 1 2
1 1
1
1
0 0 0 0
s
s
p s v
s
Q m h m'u' w m h m"u"
Q ,m' , w ,m
m h m"u"
m m"
h u"
C T C T"
T" γT
Hence(A)is thecorretanswer
82. (A) we have
1 2 1 1 2 25
0
H x x and S R x lnx x lnx
we know that
G H TS
or G H T S S T
at Constant T, T
1
1 2 1 1 2 2
1 2 1 1 2 2
1 1 1 1 1 1
2
1 1 1 1 1
5
5
5 1 1 1
5 5 1 1
G H T S
G x x T R x lnx x lnx
G x x RT x lnx x lnx
G x x RT x lnx x ln x
G x x RT x lnx x ln x
1
0
Gfor G to be minimum
x
thus,
1
1
1
1 1 1
1 1
1
1 1
1 1
1 1 1 1
1
5 10
1 1
1
Gx RT x lnx
x x
RT x ln xx
here,
lnx xx lnx x lnx
x x x
lnx
1 1
1
1
1 1 1
1
1
1
1
1 1 1
1
1
1
1
1
11 1 1
11
1 1 1
1 1
5 10 1 1 1
0 5 101
0 5
ln xx ln x x
x x
xln x
x
ln x
ln x
Gx RT lnx ln x
x
xx RTln
x
on solving, we get x .
(Gate 2013)
83. Sol. 3
The degree of freedom is given as
F = C – P + 2 – r – s = 3 – 1 + 2 – 1 – 0 = 3
84. Sol. (C)
from First Law of Thermodynamics,
Q W U
U = internal energy which solely depends
only on initial and final temperature. It is
independent of path.
85. Sol. (D)
we know that, at critical point
2 2
2
40
2
TT
P P b b ac
V aV
Hence, (D) is correct answer
86. Sol. (B)
87. Sol. (A)
Given that
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300
600
6002
300
0
0
2
surr
JE K
surr
universe
E F
E F
JF K
T K, Heat transferred from system
to suurounding,
Q J
Entropy change of surrounding,
QS
T
As we know S
or S S
S S
S
88. Sol. 0.0736
We know that
1 1 2 2
2 1
2
2
1 1 0 4 0 6
2000 4 0 09 0 6
8 314 300
0 0736
E
i i
Gx ln x ln x ln
RT
x x . .
. . . ln.
ln .
(Gate 2014)
89. Sol. (B)
90. Sol. (D)
for isentropic expansion
0
PV cons tant
Taking log on both sides
In P In V
In Pnegative
In V
is positive slope of In P vs InV is negative
Hence, (C) is correct answer
91. Sol. (C)
92. Sol. (D)
93. Sol. 0.6925
Form given Antoine equation log10 = A - B
t C,
calculate vapor pressure of both component
sat
10 1
sat
1
1210log P 7
25 230
P 177.8 torr
sat
10 2
sat
2
1 2
1206for component 2, log P 6.5
25 22.3
P 43.35 torr
Given x 0.11 and x 0.89
2
1 2 1In(y ) x [2 0.6x ]
20.89 [2 0.6x0.11]
1.53
1y 4.63
2
2 1 2
2
2
s s
1 1 1 1 2 2 2 2
s
1 1 1 1
s
2 2 2 2
In(y ) x [1.7 0.6x ]
0.11 [1.7 0.6 0.89]
0.027
y 1.02
from modified Roult 's law component 1 and 2
y P x y P and y P x y P
y P x y P
y P x y P
1
1
y 0.11 4.63 177.8
1 y 0.89 1.02 43.35
0.693
(Gate 2015)
94. Sol. (A)
We know that
s s
v
PT
We have
du Tds pdv
and dg vdp sdT
u uSo, P P
v v
uT
s
g gV and S
p T
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95. Sol. (D)
we have
0 1 0 0
1
A B C
at t ,
Let fraction of A connverted
at t t
2
2
2
2
1 1
1 1
1
2750
8 314 573
1 78
1 78 0 801
B CP
A
P
O
Thus,
y yK P
y
K P P
Also,
GlnK
RT
K exp.
K .
so, . .
96. Sol. 310
We have
0 1 0 1
0 1
320 2
2 0 1 320
30
0 1 30
310
dPGiven . dP . dT
dT
P . T c (i)
Given at T K, P bar
. c
c
equation (i) becomes
P . T
T K
97. Sol. (D)
we have
U, S, and G are state variables (point
functions)
So U, S and G
Remain same between two states 1 and 2.
98. Sol. (B)
Catalyst changes the activation energy of the
reaction
Hence, (B) is correct answer.
99. Sol. 750
Given:
1 2 : Reversible adiabatic process
2 3 : Reversible isobaric process
Given
1
5
31
62 3
33
1 1 2 2
15
11 1 667
2 1 62
22
0 1
10
2
10
0 2
2 5 1 5
2 51 667
1 5
1 2
102
10
0 50
a
P v
P v
.
P . MPa
Pa
v m
P P P
V . m
C . R So C . R
.C / C .
.
for process : P V P V
PV V x
P
V . m
Work done on for process 1-2
6 6 61 1 2 2
1 2
1 2
2 3
6
0 1 10 2 10 10 0 5
1 0 667
450
2 3
10 0 2 0 5
300
P V P V . X x x x .w
.
w kJ
work done for process
w P V
X( . . )
kJ
Net work done = 450+350=750 kJ
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100. Sol. (D)
Given R R
Pg VdP
RT RT0
1
0
34 6
1
1
11
0 10 0 2 10
20
R g
R
RP
R
R
ZRT RT RTwe know, V V V (Z )
P P P
V (Z )or
RT P
BP (Z ) BAnd Z
RT P RT
g Bso, dp
RT ERT
mg B(P ) x . x Pa
mol
g J / mol
101. Sol. 27.52
The general VLE equation
For component 1
s
1 1 1 1 1
s
2 2 2 2 1
y P x P ............................eq.1
y P x P ............................eq.2
i iat azeotrope y x
Equation 1 divides by Equation 2
s
1 1 1 1 1
s
2 2 2 2 2
y P x P
y P x P
22
21
Ax
Ax
0.9P 70e
0.9P 30e
2 22 1
A(x x )30e
70
2 22
Ax 2.12x0.70.9P 70e 70 e
P . bar27 52
(Gate 2016)
102. Sol.
Infinitely dilute solution of component (1)
1 20 1 x & x
So 2 21 2 60 1 100 0 1 h x ( ) x x( )
1 58h
103. Sol. 0.396
From Raoult’s law
. vi ii
p x p
& we’
i i
i
p pyi
p p
Mol fraction of benzene in vapor phase is
given by0 2 92
0 3960 2 92 0 8 35
V
B B BB V T
B B T Ti
x ppy
x P x pp
..
. .
104. Sol. 373
We know that
1.5irr revW W
(Change in I.E.)irr = 1.5 (change in I.E.)rev
V V
V
C (T T ) . C (T T )
T T . C (T T )
2 1 2 1
2 1 2 1
1 5
1 5
P
PT T . (T T )
1
2
12 1 1 11 5
..
T .
T K
2771 277
2
2
6300 1 5 300 1 73
3
373
105. Sol. 400
We know that
0 1
1 0
( )
RTP
v b
P v b RT
RTv
PRT
b b TP
Rb T b
P
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1 0 1 0
T P
h vv T
P T
R Rh T b T b b
P P
0
0
5 6
( )
4 10 (15 5) 10 400 /
T T
f i f i TT
dh b dP
h h b P P
J mol
106. Sol. 1.647
idE ggg
RT
g
RT
g
RT
g idE
1 1 2 2 1 1 2 2
1 2
1 2 1 2 1 1 2 23
3 0 4 0 6 0 4 1 0 6 2
0 4 0 4 0 6 0 6
E id
Ei i i i
E
g g g
RT RT RT
x g RT x lnxg g
RT RT RT
x g x g RT x lnx x lnxg g
RT RT RT
g ggx x x x x lnx x lnx
RT RT RT
g. . . .
RT
. ln( . ) . ln( . )
1 647 g
.RT
(Gate 2017)
107. Sol. (C)
For gas M; P = 25 bar, Pc = 75 bar
25 1
75 3
r
c
PP
P
For Gas N; P = 75 bar, PC = 225 bar
75 1
225 3
rP
For Gas M; T = 300 K, TC = 150 K, Tr =
2C
T
T
For Gas N; T = 1000 K, TC = 500 K, Tr =
2C
T
T
Compressibility factor, Z = k r
r
P
T
1
3
2 61
3
2 6
m
n m n
KK
Z
KK
Z Z Z
108. Sol. (D)
109. Sol. 14.9
7 7 7g g
, .RT RT
As we know
R
i
x
f gexp
P RT
7 7 7
0 7 0 7
30 0 7 14 9
R
i
x
R
ig
R
i
i
f gexp
p RT
g g g.
RT RT RT
fg. p ( . )
RT Pf exp ( . ) . bar
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110. Sol. 2511.4
As we know 1
1
T
dv( )
V dp
For isothermal process pv = const
Pdv +Vdp = 0 1
dv V
dp P
From equation
0
1
1
1 110P Pa
P
At constant temperature
111. Sol. 0.91
1000 0 92H bar, . for dilute solution
We can use Henry law for solute Hx = yP
1000 x = 0.92 (1-0.01) (10)
Here, y and x are mole fraction of solute in
gas liquid respectively x = 9.108 x 10-3
Mole percentage of solute in liquid phase =
100 (9.108 10-3) = 0.91
Gate 2018
112. Sol. 102.375
113. Sol (C)
114. Sol. 368.166
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115. Sol.