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BASIC CONCEPTS PREPARED BY
WORKSHEET HANDOUT 1 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
1
MEASUREMENT AND
UNIT CONVERSION (8)
Q 1) Change each of the following
measurements to one in which the unit has
an appropriate SI prefix.
a) 4.54 x 10-9 g b)3.76 x 10
3 m
c)6.34 x 10-6 g d) 1.09 x 10
-9 g
e) 9.01 x 10-3 s
Q2) Carry out the following temperature
conversions.
a) 23.5 °C to °F b) 98.6 °F to °C
c) 212°C to °F d) 173.9 °F to °C
e) -98.0 °C to °F f) -10.0 °F to °C
Q3) Make the following temperature
conversions.
a) The high temperature record for the
continent of Africa is 136 °F, recorded at
Azizia, Libya, in 1922. What is this
temperature in degrees Celsius?
b) In Martian water, the temperature at the
poles drop to -120°C, freezing water vapor
and carbon dioxide from the atmosphere.
What is this temperature in degrees
Fahrenheit?
Q 4) Answer the following temperature
scale questions.
a) A candy recipe calls for heating a sugar
mixture to the “soft ball” stage (234 to 240
°F). Can a laboratory thermometer with a
range of -10 to 110 °C be used for this
measurement?
b) At what temperature do the Fahrenheit
and Celsius readings have the same
numerical value? Can they have the same
value at more than one temperature?
Q 5) Carry out the following conversions.
a)50.0 km to meters b)546 mm to meter
c) 98.5 kg to grams d)47.9 ml to liters
e) 5781JS to ms f) 237 mm to cm
Q6) Carry out the following conversions.
a) 87.6 µg to kg b) 1.00 h to µs
c) 0.0962 km/min to
m/s
d) 55 km/h to m/min
e) 87.4 cm2 to mm
2 f) 46.4 m
3 to liters
Q7) Arrange the following in order of
increasing length (shortest first):
(1) l.21-m chain, (2) 75-in. rope,
(3) 3-ft-5-in. ratllesnake, (4) a yardstick.
Q8) Arrange the following in order of
increasing mass (lightest first):
(1) 5-lb bag of potatoes
(2) 1.65 kg cabbage
(3) 2500 g sugar.
DENSITY (13)
Q9) A 25.0-ml sample of liquid bromine has
a mass 78.0 g. What is the density of the
bromine?
Q10) What is the density of a salt solution if
50.0 ml has a mass of 57.0 g?
Q11) Some metal chips having a volume of
3.29 cm3 are placed on a piece of paper and
weighed. The combined mass is found to be
18.43 g. The paper itself weighs 1.2140 g.
Calculate the density of the metal to the
proper number of significant figures.
Q12) A glass container weighs 48.462 g. A
sample of 4.00 ml of antifreeze solution is
added, and the container plus the antifreeze
weigh 54.51 g. calculate the density of the
antifreeze solution to the proper number of
significant figures.
BASIC CONCEPTS PREPARED BY
WORKSHEET HANDOUT 1 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
2
Q13) A rectangular block of lead is 1.20 cm
x 2.41cm x 1.80 cm and has a mass of 59.01
g. Calculate the density of lead.
Q14) A rectangular block of gold-colored
material measures 3.00 cm x 1.25 cm x 1.50
cm and has a mass of 28.12 g. Can the
material be gold? The density of gold is 19.3
g/ml.
Q15) What is the mass in grams, of 30.0 ml
of glycerol (a syrup made from pomegranate
juice), which has a density of 1.32 g/ml?
Q16) What is the mass in kg, of 2.75 L of
the liquid glycerol, which has a density of
1.26 g/ml?
Q17) What is the volume of an 898-kg piece
of cast iron (d = 7.76 g/cm3)? If the iron is
formed into a cylindrical bar with a base
area of 1.50 cm2, how long is the bar?
Q18) What is the volume of 5.79 mg of gold
(d = 19.3 g/ml)? If the gold is hammered
into a gold leaf of uniform thickness with an
area of 44.6 cm2, what is the thickness of the
gold leaf?
Q19) A box with a base 0.80 m on a side
and a height of 1.20 m is filled with 3.2 kg
of expanded polystyrene packing material.
What is the bulk density, in g/cm-1 of the
packing material? (The bulk density
includes the air between the pieces of
polystyrene foam.)
Q20) Hylon VII, a starch-based substitute
for polystyrene packing material, has a bulk
density of 12.8 kg/m3. What mass, in grams,
of the material is needed to fill a volume
of2.00 ft3?
Q21) Which of the following items would
be most difficult to lift onto the back of a
pick up truck:
(1) A 100-lb bag of potatoes
(2) A 15-gal plastic bottle filled with water
(3) A 3.0 L flask filled with mercury
(density 13.6 g/cm3)
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
1
MOLECULAR WEIGHTS
FORMULA WEIGHTS (2)
Q1. Calculate the molecular weight or
formula weight of each of the following.
a) C6H5Br b) H3PO4
c) K2Cr207 d) AI2(SO4)3.18H20
Q2. Calculate the molecular weight or
formula weight of each of the following.
a) (NH4)3PO4 b) Na2S2O3
c) C2H5NO2 d) Fe(NO3)3.9H2O
AVOGADRO’S NUMBER &
MOLAR MASSES (3)
Q3. Calculate the average mass in grams of
an atom of:
a) silicon b) copper
c) rhodium d) cobalt
e) strontium f) lead
Q4. Calculate the mass, in grams, of each of
the following:
a) 0.00500 mole MnO2
b) I.12 mole CaH2
c) 0.250 mole C6H1206
d) 4.61 mole AICI3
e) 0.615 mole of chromium (III) oxide
f) 0.158 mole of iodine pentafluoride
Q5. Calculate the amount, in moles, of each
of the following:
a) 98.6 g HNO3 b) 9.45 g CBr4
c) 9.11 g FeSO4 d) 11.8 g Pb(NO3)2
e) 16.3 g of sulfur hexafluoride
f) 25.4 g of lead (II) acetate
g) 35.6 g of iron (III) chloride heptahydrate
h) 75.3 g of cobalt (II) chlorate hexahydrate
PERCENTAGE
COMPOSITION AND
EMPIRICAL FORMULA (9)
Q6. Calculate the mass percent of each
element in each of the following
compounds:
a) BaSiO3 b) C6H5NO2
c) Mg(HCO3)2 d) Al(BrO3)3.9H2O
e)C3H8O f)(NH4)2SO4
g)C6H8N2 h)Ba(ClO4)2.3H2O
Q7. The empirical formula of para-
dichlorobenzene, used as a moth repellent, is
C3H2CI. The molecular weight of the
compound is 147 u. What is the molecular
formula?
Q8. The empirical formula of apigenin, a
yellow dye for wool, is C3H2O. The
molecular weight of the compound is 270 u.
What is the molecular formula?
Q9. Chloroform, an organic solvent, is
10.05% C, 0.84% H and 89.10% Cl by
mass. Determine its empirical formula.
Q10. Urea, used as a fertilizer and in the
manufacture of plastics, is 20.00 % C, 6.71
% H, 46.65% N and 26.64% 0 by mass.
Determine its empirical formula.
Q11. Resorcinol, used in manufacturing
resins, drugs and other products, is 65.44%
C, 5.49% H and 29.06% O by mass.
Determine its empirical formula. The
molecular weight of resorcinol is 110 u.
What is its molecular formula?
Q12. Sodium tetrathionate is formed when
sodium thiosulfate reacts with iodide.
�a2S2O3 + I2
> �axSyOz + �aI
(Not balanced)
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
2
Its composition is 17.01% Na, 47.46% S and
35.52% O by mass. Determine its empirical
formula. The formula weight of sodium
tetrathionate is 270 u. What is its actual
formula?
Q13. A 0.1204-g sample of a carboxylic
acid is burned in oxygen to yield 0.2147 g
Co2 and O.0884g H2O. Calculate the mass
percentages of carbon, hydrogen and oxygen
in the compound.
Q14. A 0.0989-g sample of an alcohol is
burned in oxygen to yield 0.2160 g CO2 and
0.1194 g H2O. Calculate the mass
percentages of carbon, hydrogen and oxygen
in the compound.
STOICHIOMETRY OF
CHEMICALREACTIONS (9)
Q15. Consider the equation for the
combustion of octane in oxygen.
2 C8H18 + 25 02
> 16 CO2 + 18 H20
(a) How many moles of C02 are produced
when 2.0 x 1010 moles of C8H18 is burned?
(b) How many moles of oxygen are required
to burn 4.4 x 1010 moles of C8H18?
(c) How many moles of H2O are produced
when 2.0 x 108 moles of C8H18 is burned?
(d) How many moles of C02 are produced
when 4.0 x 108 moles of O2 is consumed?
Q16. Given the equation:
�2 + H2
> �H3 (Not balanced)
(a) How many grams of ammonia can be
made from 440 g H2?
(b) How many grams of hydrogen are
needed to react completely with 892 g N2?
Q17. What mass of oxygen, in grams, can
be prepared from 24.0 g H2O2?
H2O2
> H2O + O2 (Not balanced)
Q18. Toluene and nitric acid are used in the
production of trinitrotoluene (TNT), an
explosive.
C7H8 + H�O3
> C7H5�3O6 + H2O
Toluene TNT
(Not balanced)
(a) What mass of nitric acid is required to
react with 454 g C7H8?
(b) Calculate the mass of TNT that can be
made from 829 g C7H8.
Q19. How many kilograms of quicklime
(calcium oxide) can be made when 4.72 x
109 g of limestone (calcium carbonate) is
decomposed by heating?
CaCO3
> CaO + CO2
Q20. How many grams of nitric acid can be
made from 971 g of ammonia?
�H3 + O2
> H�O3 + H2O
(Not balanced)
Q21. In an oxyacetylene welding torch,
acetylene (C2H2) burns in pure oxygen with
a very hot flame.
C2H2 + O2
>C02 +H2O (Not balanced)
How many grams of oxygen are required to
react with 52.0 g C2H2?
Q22. Kerosene is a mixture of hydrocarbons
used in domestic heating and as a jet fuel.
C14H30 + O2
> CO2 + H2O
(Not balanced)
(a) How many grams of CO2 are produced
by the combustion of 1.00 gal of kerosene?
Assume that kerosene can be represented as
C14H30 and that it has a density of 0.763
g/ml. (l gal = 3.785 L)
(b) How many milliliters of kerosene must
be burnt to produce 1.00 kg CO2?
Q23. Ordinary chalkboard chalk is a solid
mixture with limestone (CaCO3) and
gypsum (CaSO4) as its principal ingredients.
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
3
The limestone dissolves in dilute HCI , but
the gypsum does not.
CaCO3 + HCl
> CaCI2 + CO2 + H2O
(Not balanced)
(a) 5.05-g piece of chalk that is 72.0%
CaCO3 dissolved in excess HCl , what mass
of CO2 will be produced?
(b) What is the mass percent CaCO3 present
if a 4.38-g piece of chalk yields 1.31 g CO2
when reacts with excess HCI?
LIMITING REACTANT AND
YIELD CALCULATIONS (7)
Q24. Lithium hydroxide absorbs carbon
dioxide to form lithium carbonate and water.
2 LiOH + CO2
> Li2CO3 + H2O
If a reaction vessel contains 0.150 mole of
LiOH and 0.080 mole of CO2 which
compound is the limiting reactant? How
many moles of Li2CO3 can be produced?
Q25. Boron trifluoride reacts with water to
produce boric acid H3BO3 and fluoroboric
acid (HBF4).
4 BF3 + 3 H2O
> H3BO3 + 3 HBF
If a reaction vessel contains 0.496 mole BF3
and O.313 mole H2O which compound is the
limiting reactant? How many moles of HBF4
can be produced?
Q26. Propane C3H8 burns in oxygen to
produce carbon dioxide and water. If a
reaction vessel contains 4.81 g C3H8 and
16.4 g of which compound is the limiting
reactant? What are the maximum number
grams of carbon dioxide that can be
produced?
Q27. Butane, C4H10 burns in oxygen to
produce carbon dioxide and water. If a
reaction vessel contains 8.37 g C4H10 and
31.9 g O2 which compound is the limiting
reactant? What are the maximum number
grams of carbon dioxide that can be
produced?
Q28. Calculate the theoretical yield of ZnS,
in grams, that can be made from 0.488 g Zn
and 0.503 g S8.
8 Zn + 58
> 8 ZnS
If the actual yield is 0.606 g ZnS, what is the
percent yield?
Q29. Calculate the theoretical yield of
C2H5Cl, in grams, that can be made from
11.3 g of ethanol and 3.48 g PCl3.
3 C2H5OH + PCl3
>
3 C2H5Cl + H3PO3
If the actual yield is 1.24 g C2H5Cl, what is
the percent yield?
Q30. A student prepares ammonium
bicarbonate by the reaction:
�H3 + CO2 + H2O
>�H4HCO3
He uses 14.8 g of NH3 and 41.3g of CO2.
Water is used in excess. What is his actual
yield of ammonium bicarbonate hi obtains
74.7 % yield in the reaction?
SOLUTION
STOICHIOMETRY (20)
Q31. Calculate the molarity of each of the
following solutions:
a) 6 mole HCl in 2.5 L of solution
b) 0.007 mole Li2CO3 in 10.0 ml of solution
c) 2.50 mole H2SO4 in 5 l of solution
d) 0.20 mole C2H5OH in 18.4 ml of solution
e) 8.9 g H2SO4 in 100 ml of solution
f) 439 g of C6H12O6 in 1.25 L of solution
g) 44.3 g KOH in 125 ml of solution
h) 2.46 g H2C2O4 in 750 ml of solution
Q32. How many grams of solute are needed
to prepare each of the following solutions?
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
4
a) 2 L of 1.0 M NaOH
b) 10 ml of 4.25 M C6H12O6
c) 250 ml of 2.50 M K2Cr2O7
d) 20 ml of 0.00100 M KMnO4
Q33. How many milliliters of 6 M NaOH
are required to contain 1.25 mole NaOH?
Q34. How many milliliters of 2.5 M NaOH
are required to contain 1.05 mole NaOH?
Q35. How many milliliters of 0.0250
KMnO4 are required to contain 8.10 g of
KMnO4?
Q36. How many milliliters of 4.25 M
C6H12O6 are required to contain 205g of
C6H12O6?
Q37. How many milliliters of 12 M HCl are
required to make 2 L of 1.0 M HCl?
Q38. How many milliliters of 8.89 M HBr
are required to make 2 L of 1.0 M HBr?
Q39. If 25.0 ml of 1.04 M Na2CO3 is diluted
to 0.50 L, what is the molarity of Na2CO3 in
the diluted solution?
Q40. If 50 ml of 19.1 M NaOH is diluted to
2 L, what is the molarity of NaOH in the
diluted solution?
Q41. Which of the following is the
approximate molarity of a solution obtained
by mixing 0.1 L of 0.100 M NH3 and 0.200
L of 0.2 M NH3?
Q42. A stock bottle of potassium hydroxide
solution indicates that the solution is 67%
HNO3 by mass and has a density of 1.40
g/ml. Calculate the molarity of the solution.
Q43. A stock bottle of potassium hydroxide
solution indicates that the solution is 50% by
mass and has a density of 1.52 g/ml.
Calculate the molarity of the solution.
Q44. Calculate the molarity of an HCl
solution if 20 ml of it requires 33.22 ml of
0.1503 M NaOH for its neutralization.
�aOH + HCl
> �aCl + H2O
Q45. Calculate the molarity of an HNO3
solution if 30 ml of it requires 18.34 ml of
0.1044 M KOH for its neutralization.
KOH + H�O3
> K�O3 + H2O
Q46. Calculate the molarity of a Ca(OH)2
solution if 18.5 ml of it requires 28.27 ml of
0.01025 M HCl for its neutralization.
Ca(OH)2 + 2 HCl
> CaCl2 + 2 H2O
Q47. Calculate the molarity of a H2C2O4
solution if 12.5 ml of it requires 25.72 ml of
0.0995 M NaOH for its neutralization.
H2C2O4+ 2 �aOH
>
�a2C2O4 + 2 H2O
Q48. How many milliliters of 0.100 M
H2SO4 are required to react with 10.32 ml of
0.4042 M NaHCO3?
H2SO4+ 2 �aHCO3
>
�a2SO4 + 2 H2O + CO2
Q49. How many milliliters of 0.1104 M
H2SO4 are required to react with 30.07 ml
of 0.08872 M Ba(OH)2?
H2SO4+ Ba(OH)3
>
BaSO4 + 2 H2O
Q50. A solution is prepared by dissolving 4
g NAOH in 25 g of water. What mass of
H2SO4 is required in 500g of water to
prepare the solution of same molarity as that
of NaOH solution?
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
NSTC-6 PREPARATION PROGRAMME | AGA KHAN HIGHER SECONDARY SCHOOL,
KARACHI.
5
MISCELLANEOUS 1 (23)
Q51. Calculate the molecular weight of
sulphur hexafluoride, SF6, a gas used as an
electric insulator in high-voltage equipment.
Q52. Calculate the formula weight of
ammonium sulfate, a fertilizer commonly
used by home gardeners.
Q53. Calculate the mass, in grams, of 0.250
mole of Na.
Q54. Calculate the number of moles of CO2
present in a 225g sample of the gas.
Q55. How many Cl- ions are present in
1.38g MgCl2?
Q56. What is the mass of a sodium atom, in
grams?
Q57. Calculate the mass percent of each
element in ammonium hydroxide (NH4OH).
Q58. What mass of nitrogen, in grams, is
present in 46.34 g ammonium nitrate?
Q59. Phenol, a general disinfectant, is
76.57% C. 6.43% H, and 17.00% O.
Determine its empirical formula.
Q60. Diethylene glycol, used as an
antifreeze, is 45.27% C, 9.50% H and
45.23% O. Determine its empirical formula.
Q61. The empirical formula of
hydroquinone, a chemical used in
photography, is C3H3O, and its molecular
weight is 110u. What is its molecular
formula?
Q62. A 0.1000-g sample of a compound of
C, H and O is burned in oxygen to yield
0.1953g CO2 and 0.1000g H2O. Its
molecular weight had previously been found
to be 90 u.
a. Calculate the mass percent composition
of the compound.
b. What is the empirical formula of the
compound?
c. What is its molecular formula?
Q63. When 0.105 mole propane is burned
in a rich supply of oxygen, how many moles
of oxygen are consumed.
C3H8 + 5O2
> 3CO2 + 4 H2O
Q64. Ammonia, NH3, a common fertilizer,
is made by causing hydrogen and nitrogen to
react at a high temperature and pressure.
How many grams of ammonia can be made
from 60.0g of hydrogen?
Q65. A sheet of iron with a surface area of
525 cm2 is covered with a coating of rust
that has an average thickness of 0.0021 cm.
What mass of a hydrochloric acid solution
that is 15% HCl by mass is required to clean
the surface of the metal by dissolving the
rust? Assume that the rust is iron (III) oxide
and that its density is 5.2 g/cm3.
Fe2O3 + 6HCl
> 2FeCl3 + 3H2O
Q66. Potassium iodide is used as a dietary
supplement to prevent goiter, an iodine
deficiency disease. It is prepared by the
reaction of hydrogen iodide and potassium
hydrogen carbonate.
HI + KHCO3
> KI + H2O + CO2
a. How many grams of KI can be made by
mixing 481 g HI and 318 g KHCO3?
b. Which reactant is in excess, and how
many grams of it remain after the
reaction?
CHEMICAL LANGUAGE PREPARED BY
WORKSHEET HANDOUT 2 OSAMA HASAN
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Q67. Ethyl acetate is a solvent used as
fingernail polish remover. How many grams
of acetic acid are needed to prepare 252 g of
ethyl acetate if the expected percent yield is
only 85.0%? Assume that the other reactant,
ethyl alcohol, is present in excess. The
equation for the reaction, carried out in the
presence of H2SO4, is
CH3COOH + C2H5OH
>
CH3COOC2H5 + H2O
Q68. What is the molarity of a solution in
which 333g of potassium hydrogen
carbonate is dissolved in enough water to
make 10.0L of solution?
Q69. How many grams of NaOH are
required to prepare 0.500 L of 6.67M
NaOH?
Q70. A stock bottle of aqueous ammonia
indicates that the solution is 28.0% NH3 by
mass and has a density of 0.898 g/ml.
calculate the molarity of the solution.
Q71. How many milliliters of a 2.00M
CuSO4 stock solution would you use to
prepare 0.250L of 0.400M CuSO4?
Q72. A flask contains 25.00 ml of H2SO4 of
unknown concentration. Titration of the
sample requires 25.20 ml of 0.1000 M
NaOH for neutralization. What is the
molarity of the sulfuric acid solution?
Q73. A flask contains 20.00 ml of 0.1030 M
HCl. What Volume of 0.2010M NaOH must
be added to just neutralize the acid?
�aOH + HCl
> �aCl + H2O
CHEMICAL LANGUAGE PREPARED BY
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MISCELLANEOUS 2 (25)
Q74. Calculate, to five significant figures,
the molecular weight of each of the
following compounds.
a) C6H12Br2 b) C2H2Cl2O2
c) H5P3O10 d) C6H4Cl2O2S
Q75. Calculate the formula weight of each
of the following compounds.
a) K2SbF5 b) barium bromate
c) iron(III) phosphate d) NaB(C6H5)4
Q76. Calculate the amount, in moles, of
each of the following:
a) 3.17g Fe b) 76.0 mg of H3PO3
c) 1.65 x 103 kg C4H10 d) 1.99 g of K2CrO4
Q77. Calculate the mass, in grams of each
of the following.
a) 55.5 mole H2O b) 0.0102 mole C4H10O
c) 2.45 x 10-4 mole of
C2H6
d) 2.13 mole of HNO3
Q78. Calculate the number of:
(a) Atom in 6.17g Ca
(b) Molecules in 0.0100g N2
(c) Molecules in 18.5 g butane, C4H10
(d) Atoms in 215 g of sucrose C12H22O11
Q79. Calculate the average mass in grams of
(a) A helium atom
(b) A bismuth atom
(c) A carbon tetrachloride (CCl4) molecule
(d) A propane molecule.
Q80. Calculate the mass percent of each
element in
(a) Ammonium sulfate
(b) Urea, CO(NH2)2.
Which compound has the greatest mass
percent nitrogen: ammonium sulfate or
urea?
Q81. People with hypertension (high blood
pressure) are advised to limit the amount of
sodium (actually sodium ion, Na+) in their
diets. Calculate the mass, in mg, of Na+ in
5.00g of sodium hydrogen carbonate
(sodium bicarbonate).
Q82. Mebutamate, a diuretic “water pill”
used to treat hypertension, is 51.70% C,
8.68% H, 12.06% N and 27.55% O.
determine its empirical formula.
Q83. Trinitrotoluene (TNT), an explosive, is
37.01% C, 2.22% H, 18.50% N, and 42.27%
O. determine its empirical formula.
Q84. Ethylene (molecular weight: 28.0u),
cyclohexane (84.0u), and 1-pentene (70.0u)
all have the empirical formula CH2. Give the
molecular formula of each compound.
Q85. A 0.3629-g sample of
tetrahydrocannabinol, a compound of C, H,
and O and the principal active component of
marijuana, is burned in oxygen to yield
1.067 g of carbon dioxide and 0.3120 g of
water.
a. Calculate its mass percent composition.
b.Calculate its empirical formula.
Q86. For the combustion of propane in
example3.16:
a. How many moles of carbon dioxide are
formed when 0.529 mole of C3H8 is
burned?
b.How many moles of water are produced
when 76.2 mole C3H8 is burned?
c. How many moles of carbon dioxide are
produced when 1.010 mole of O2 is
consumed?
Q87. How many grams of magnesium metal
are required to reduce 83.6 g of titanium
(IV) chloride to titanium metal? Magnesium
chloride is other product.
CHEMICAL LANGUAGE PREPARED BY
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8
Q88. The decomposition of potassium
chlorate produces potassium chloride and
oxygen gas. How many grams of oxygen
can be made from 2.47 g of potassium
chlorate?
Q89. How many milliliters of liquid water
should be produced by the combustion in
oxygen of 775 ml of liquid octane? Assume
that the volumes of both liquids are
measured at 20 C, where the densities are
0.7025 g/ml for octane and 0.9982 g/ml for
water.
Q90. Hydrogen sulfide is a foul-smelling
gas that was extensively used at one time to
precipitate (separate from solution as solids)
metal sulfides in a laboratory scheme to
identify certain cations in aqueous solutions.
One way to produce the gas is by the time
reaction of iron (II) sulfide with
hydrochloric acid.
FeS + 2HCl
> FeCl2 + H2S
If 10.2g HCL is added to 13.2g FeS, how
many grams of H2S can be formed?
Q91. Isopentyl acetate is the main
component of banana flavoring. Calculate
the theoretical yield of isopentyl acetate that
can be obtained from 20.0 g of isopentyl
alcohol and 25.0 g of acetic acid.
CH3COOH + C5H11OH
>
CH3COO C5H11 + H2O
If the percent yield of the reaction is 90.0%,
what is the actual yield of isopentyl acetate?
Q92. How many grams of isopentyl alcohol
are needed to make 433 g of isopentyl
acetate in the reaction described in exercise
3.19 if the expected yield is 85.0%? Assume
the acetic acid is in excess.
Q93. Calculate the molarity of each of the
following solutions.
a. 18.0 mole H2SO4 in 2.00 L of solution
b.3.00 mole KI in 2.39L of solution
c. 0.206 mole HF in 752 ml of solution
d.0.522g HCl in 0.592 L of solution
e. 4.98g C6H12O6 in 24.7 ml of solution
Q94. How many grams of potassium
hydroxide are required to prepare each of
the following solutions?
a) 2 L of 6M KOH b) 100 ml of 1M KOH
c) 10 ml of 0.1M KOH d) 33 ml of 2.5M KOH
Q95. A stock bottle of aqueous formic acid
indicates that the solution is 90.0% HCOOH
by mass and has a density of 1.20 g/ml.
calculate the molarity of the solution.
Q96. How many milliliters of a 10.15M
NaOH stock solution would you use to
prepare 15.0L of 0.315M NaOH?
Q97. A flask contains 20.00 ml of KOH of
unknown concentration. Titration of the
solution requires 15.62 ml of 0.1104M
H2SO4.
2KOH + H2SO4
> K2SO4 + 2H2O
Calculate the molarity of the KOH.
Q98. How many milliliters of 0.100M
AgNO3 are required to react completely with
750.0 ml of 0.0250M Na2CrO4?
2Ag�O3 + �a2CrO4
>
Ag2CrO4 + 2�a�O3
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Q1. Predict atleast five general properties of the compounds occupying the indicated positions
in periodic table:
A
C
K B I
H D
L J
G M F
E
Q2. Arrange each set of elements in order of
increasing atomic radius that is, from
smallest to largest:
a) Mg, Si, S b) As, N, P c) As, Se, Sb
Q3. Arrange each set of elements in order of
decreasing atomic radius:
a) Be, F, N b) Ba, Be, Ca
c) Cl, F, S d) Ca, K, Mg
Q4. Arrange the following species in order
increasing radius: S2-, Ca
2+, Mg
2+, K
+, Se
2+.
Q5. Arrange the following species in order
decreasing radius: Br-, Rb
+, Se
2-, Sr
2+, Y
3+.
Q6. Arrange each set of the elements in
order of increasing first ionization energy:
a) Mg, Si, S b) As, N, P
c) As, Se, Sb
Q7. Arrange each set of elements in order of
decreasing first ionization energy:
a) Be, F, N b) Ba, Be, Ca
c) P, F, S d) Ca, K, Mg
Q8. In each set, indicate which the more
metallic element is:
a) Ba, Ca b) Sb, Sn
c) Ge, S
Q9. In each sets, indicate the more non-
metallic element:
a) O,P b) As, S c) P, F
Q10. Without referring to any tables or
listing, mark an appropriate location for
each of the following in the blank periodic
table provided:
a) The fourth period noble gas.
b) A fifth period element whose atoms have
three unpaired electrons.
c) The d-block element having one 3-d
electron
d) A p-block element that is a metalloid.
e) A metal that forms the oxide M2O3.
DESCRIPTIVE
QUESTIONS (4)
Q1. Describe the following periodic trends
and their effect on the properties of the
elements in the modern periodic table:
� Atomic/Ionic Radius � Ionization Potential
� Electron Affinity � Electronegativity
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� Electropositivity � Density
� M.P and B.P � Bond Formation
� Hardness � State
� Nature � Electronic Configuration
Q2. Discuss the factors on which the
following periodic trends depend:
� Atomic/Ionic Radius � Ionization Potential
� Electron Affinity � Electronegativity
� Electropositivity � Density
� M.P and B.P � Bond Formation
� Hardness � State
� Nature � Electronic Configuration
Q3. Discuss the general properties of the
following groups and blocks:
� Group I-A � Group II-A
� Group III-A � Group IV-A
� Group V-A � Group VI-A
� Group VII-A � Group VIII-A
� Transition elements
Q4. Describe the characteristics you can
predict about an element by knowing just its
atomic number of position in periodic table.
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DESCRIPTIVE
QUESTIONS (11)
Q1. Describe what a gas is like at the
molecular level?
Q2. Why don’t the molecules of a gas settle
to the bottom of the container?
Q3. Give a kinetic molecular explanation of
the origin of gas pressure.
Q4. State Boyle's law in words and as a
mathematical equation.
Q5. What is the advantage of storing gases
under high pressure (for example, oxygen
used in respiration therapy)?
Q6. What effect will the following changes
have on the volume of a fixed amount of
gas?
(a) An increase in pressure at constant
temperature
(b) A decrease in temperature at constant
pressure
(c) A decrease in pressure coupled with an
increase in temperature
Q7. What effect will the following changes
have on the pressure of a fixed amount of a
gas?
(a) An increase in temperature at constant
volume
(b) Decrease in volume at constant
temperature
(c) An increase in temperature coupled with
a decrease in volume
Q8. According to the kinetic-molecular
theory,
(a) What change in temperature is occurring
if the molecules of a gas begin to move
more slowly, on average?
(b) What change in pressure occurs when
the walls of the container are struck less
often by molecules of the gas?
Q9. Container A has twice the volume but
holds twice as many gas molecules as
container B at the same temperature. Use the
kinetic-molecular theory to compare the
pressures in the two containers.
Q10. For each of the following, indicate in
which container the gas would be expected
to have higher density.
(a) Containers A and B have the same
volume and are at the same temperature, but
the gas in A is at high pressure higher
pressure.
(b) Containers A and B are at the same
pressure and temperature, but the volume of
A is greater than that of B.
(c) Containers A and B are at the same
pressure and volume, but the gas in A is at a
higher temperature.
Q11. Interpret what we mean by temperature
in terms of the kinetic-molecular theory.
PRESSURE (7)
Q12. Calculate the height of a mercury
column that exerts a pressure of 4.36 atm.
Q13. Calculate the height of a mercury
column that exerts a pressure.of213 torr.
Q14. Carry out the following conversions
between pressure units.
a) 721 torr to atm b) 849 torr to atm
c) 985 atm to mmHg
Q15. Carry out the following conversions
between pressure units.
a) 642 torr to kPa b) 105.7 kPa to torr
c) 4.00 atm to mmHg
Q16. A manometer is filled with an oil that
has a density of 0.798 g/ml. Calculate the
gas pressure measured by the manometer if:
a) Barometric pressure is 755 mmHg and
the oil column on the side of the gas flask.
hclosed is 44 mm lower than on the open side,
hopen. b) Barometric pressure is 735 torr and the
oil column on the side of the gas flask,
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hclosed is 22.3 cm higher than on the open
side, hopen.
Q17. Calculate the heights of columns of
carbon tetra bromide (d = 3.42 g/ml) that
exert the same pressures as a column of
mercury (d = 13.6 g1ml) that is 760 mm
high and a column of water (d = 1.00 glml)
that is 25.5 cm high.
Q18. City fire codes specify the water
pressure that must be maintained at the end
of a water line for example. 35.5 Ib/in2.
Calculate the height of a water column that
exerts a pressure of 35.5 Ib/in2 (Him: 1 atm
= 14.7 Ib/in.2.)
BOYLE’S LAW (6)
Q19. A sample of helium occupies 521 ml
at 1572 torr. Assume that the temperature is
held constant and determine (a) the volume
of the helium at 752 torr; (b) the volume of
the helium at 3.55 atm; (c) the pressure in
torr, if the volume is changed to 315 ml (d)
the pressure in atm if the volume is changed
to 2.75 ml.
Q20. A decomposition chamber used by
deep sea divers has a volume of 10.3 m3
and
operates at an internal pressure of 4.50 atm.
How many cubic meters would the air in the
chamber occupy if it were at normal
atmospheric pressure, assuming no
temperature change?
Q21. A novel energy storage system
involves storing air under high pressure.
(Energy is released when the air is allowed
to expand) How many cubic feet of air
measured at standard atmospheric pressure
of 14.7 pounds per square inch (psi), can be
compressed into a 19-million-ft3
underground cavern at a pressure of 1070
psi?
Q22. Oxygen used in respiratory therapy is
stored at room temperature under a pressure
of 1.50 x 102 atm in gas cylinders with a
volume of 60.0 L.
a) What volume would the gas occupy at a
pressure of 750.0 torr? Assume no
temperature change.
b) If the oxygen flow to the patient is
adjusted to 8.00 L per minute, at room
temperature and 7500 torr, how long will
the tank of gas last?
Q23. A gas is confined in an upright
cylinder closed off by a piston that has a
diameter of 15.0 em. The volume of the gas
is 1.20 L at standard atmospheric pressure.
What total pressure must be exerted on the
piston to cause it to move down 5.25 cm?
Q24. The pressure within a 2.25-L balloon
is 1.10 atm. If the volume of the balloon
increases to 7.05 L. what will be the final
pressure within the balloon, if the
temperature does not change?
CHARLES’ LAW (4)
Q25. A gas at a temperature of 100 °C
occupies a volume of 154 ml. What will the
volume be at a temperature of 10 0 °C,
assuming no change in pressure'?
Q26. A balloon is filled with helium. Its
volume is 5.90 L at 26°C. What will be its
volume at -78 °C, assuming no pressure
change?
Q27. A 567-ml sample of a gas at 305°C
and 1.20 atm is cooled at constant pressure
until its volume becomes 425 ml. What is
the new gas temperature?
Q28. A sample of gas at STP is to be heated
at constant pressure until its volume triples.
What is the new gas temperature?
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AVAGADRO’S LAW AND
MOLAR VOLUME AT S.T.P (4)
Q29. Which of the following gas samples at
STP contains the greatest number of
molecules?
a) 5.0 g H2 b) 50 L SF6
c)1.0 x 1024
molecules of CO2
Q30.a) How many molecules are present in
475 ml of CO2 at STP?
b) What is the volume occupied by 3.50 x
1024
SO2 molecules at STP?
Q31. What is the mass of 498 L of neon gas
at STP?
Q32. What is the volume occupied by
0.837 g of xenon gas at STP?
THE COMBINED GAS LAW (6)
Q33. A sealed can with an internal pressure
of 721 torr at 25 °C is thrown into an
incinerator operating at 755°C. What will be
the pressure inside the heated can, assuming
the container remains intact during
incineration?
Q34. A fixed amount of He exerts a
pressure of 775 mmHg in a 1.05L container
at 26°C. To what value must the
temperature be changed to reduce the gas
pressure to 725 mmHg? Assume the volume
of gas remains constant
Q35. Suppose we wish to contain a 1.00
mole sample of gas at 1.00 atm pressure and
25 °C. What volume container would we
need?
Q36. At 25°C, the pressure in a gas cylinder
containing 8.00 moles 02 is 5.05 atm. To
maintain both pressure and volume
constant, how many moles of O2 must be
released when the temperature is raised to
235°C?
Q37. If a fixed amount of gas occupies 2.53
m3
at a temperature of -15°C and 191 torr.
What volume will it occupy at 25°C and
1142 torr?
Q38. In terms of pressure (P), volume (V),
Kelvin temperature (T), and amount of gas
(n) sketch a graph of each of the following:
a) V as a function of P, with T and n held
constant
b) n as a function of P, with T and V held
constant
c) T as a function of P, with V and n held
constant
d) N as a function of T with P and V held
constant.
THE IDEAL GAS LAW (8)
Q39. Calculate the volume:
a) In liters, of 1.12 mol H2S at 62°C and
1.38 atm
b) In ml, of 6.00 x 10-3
mol of a gas at 31°C
and 661 mmHg.
Q40. Calculate the volume:
a) In ml, of 3.45 mg O2 at 24°C and 775
mmHg
b) In m3, of 6.92 kg SF6 at 100.0°C and 743
torr.
Q41. Calculate the pressure:
a) In atm, of 4.64 mol CO in a 3.96-L tank
at 29°C
b) In mmHg or 0.0108 mole CH4 in a
0.265L flask at 37°C.
Q42. Calculate the pressure:
(a) In mmHg, of 1.42 g CO2 in a 735ml
flask at -12°C
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b) In kPa, of 35.5 g N2 in a 5 .35L flask at 0
°C.
Q43. Calculate the mass:
a) In grams, of Kr in 2.22 L at 698 torr and
45°C
b) In milligrams, of CO in 7.45l at 784 torr
and 36°C.
Q44.a) If the gas present in 4.65 L at STP is
changed to temperature of 15°C and a
pressure of 756 torr, what will be the new
volume?
b) What volume will 498 ml of a fixed
amount of gas, measured at 27°C and 722
torr, occupy at STP?
Q45. The interior volume of the Hubert H.
Humphrey Metrodome in Minneapolis is
1.70 x 1010
L. The Teflon coated fiberglass
roof is supported by air pressure provided
by 20 huge electric fans. How many moles
of air are present in the dome if the pressure
is 1.02 atm at 18°C?
Q46. A hyperbaric chamber is an enclosure
containing oxygen at higher-than-normal
pressure used in the treatment of certain
heart and circulatory conditions. What
volume of O2, from a cylinder at 25 °C and
151 atm, is required to fill a hyperbaric
chamber with a volume of 4.20 x 103L to a
pressure of 3.00 atm at 17°C?
MOLAR WEIGHT
DETERMINATIONS (4)
Q47. Calculate the molecular weight of a
gas if 0.549 g occupies 211ml at 747 mmHg
and 24°C.
Q48. Calculate the molecular weight of a
gas if 0.233 g occupies 334 ml at 721 torr
and 28°C.
Q49. Calculate the molecular weight of a
liquid that, when vaporized at 98°C and 756
torr, gave 125 ml of vapour with a mass of
0.625 g.
Q50. Calculate the molecular weight of a
liquid that, when vaporized at 99°C and 716
torr, gave 25 ml of vapour with a mass of
0.625g.
GAS DENSITIES (5) Q51. Calculate the densities of each of the
following in g/dm3:
a) CO at STP
b) Ar at 1.26 atm and 235°C
c) AsH3 at STP
d) N2 at 715 torr and 98°C
Q52. At what temperature will O2 at 0.982
atm pressure have a density of 1.05 g/dm3?
Q53. At what pressure will N2 have a
density of 0.985 g/dm3 at 25°C?
Q54. What must be the molar mass of a gas
found to have a density of 2.57 g/dm3 at 25
°C and 745 torr?'
Q55. Which of the following gases is (are)
more dense than O2 at STP?
a) N2 at STP
b) CO at 0°C and 1.5 atn
c) SO2 at 300°C and 1 atm
d) H2 at 25°C and 10 atm
STOICHIOMETRY OF
GASEOUS REACTIONS (6)
Q56. How many-liters of SO3 can be
produced by the reaction of 1.15 L SO2 and
0.65 L O2, if all three gases are measured at
the same temperature and pressure?
2 S02 + 02
> 2 SO3
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Q57. What minimum volume of O2 is
required to convert 3.06 L CO to CO2, if all
three gases are measured at the same
temperature and pressure?
CO + ½O2
>CO2
Q58. How many liters of CO2 measured at
22.5°C and 743.5 mmHg are produced in
the decomposition of one metric ton (1.00 x
103 kg) of limestone?
CaC03
> CaO + CO2
Q59. What volume of O2 measured at 22 °C
and 763 torr, is consumed in the combustion
of 7.50 L of C2H6, measured at STP?
2C2H6 + 702
> 4 CO2 + 6 H2O
Q60. How many milligrams of magnesium
metal must react with excess HCl to
produce 28.50 ml of H2, measured at 26 °C
and 758 torr?
Mg + 2 HCI
> MgCl2 + H2
Q61. A 100.0 g sample of aqueous
hydrogen peroxide solution decomposes
over time, producing 2.17 L O2 and 25°C
and 755 torr.
2 H2O2
> 2 H2O + O2
What must have been the mass percent
H2O2 in the solution?
MIXTURE OF GASES (7)
Q62. Calculate the mole fraction of each
gas in the following mixtures:
a) 0.354 g Ar, 0.0521 g Ne, and O.O0419 g
Kr.
b) 1.98 g N2, 0.390 g O2 and 0.0201 g Ar.
Q63. A gas sample has 76.8 mole percent
N2, 20.1 mole percent 02 and 3.1 mole
percent CO2. If the total pressure is 762
mmHg, what are the partial pressures of the
three gases?
Q64. A sample of intestinal gas was
collected and found to consist of 44% CO2,
38% H2, 17% N2, 1.3% 02, and 0.003% CH4
by volume. What is the partial pressure of
each gas, if the total pressure in the intestine
is 818 torr?
Q65. Mixtures of helium and oxygen are
used in· scuba diving. What are the partial
pressures of the two gases in a mixture of
1.96 g He and 60.8 g O2 contained in a
5.00L tank at 25°C?
Q66. Oxygen is collected over water at
30°C and a barometric pressure of 742 torr.
What is the partial pressure of O2 in the
container?
Q67. An oxygen-helium gas sample
collected over water at 23°C exerts a total
pressure of 758 torr. Calculate the mole
fraction of water vapor in the sample.
Q68. Elodea is a green plant that carries out
photosynthesis under water.
6 CO2 + 6 H2O
> C6H12O6 + 6 O2
In an experiment some Elodea produce 1.2
ml of O2 collected over water at 743 torr
and 21°C. What mass of oxygen is
produced? What mass of glucose (C6H12O6)
is produced concurrently?
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MISCELLANEOUS 1 (23)
Q69. A Canadian weather report gives the
atmospheric pressure as 100.2 kPa. What is
the pressure in torr?
Q70. Calculate the height of a column of
water that would exert the same pressure as
a column of mercury that is 760 mm high.
Q71. Elephant seals dive to depths as great
as 1250 m. what pressure, in atm, is exerted
by water at that depth?
Q72. A cylinder of oxygen has a volume of
2.00 L. the pressure of the gas is 1360 lb/in2
at 20°C. What volume will the oxygen
occupy at standard atmospheric pressure
(14.7 lb/in.2), assuming there is no
temperature change?
Q73. A weather balloon is partially filled
with helium. On the ground, where the
atmospheric pressure is 748 torr, the volume
of the balloon is 10.0 m3. When the balloon
reaches an altitude of 5300 m, its volume is
found to be 20.2 m3. Assuming that the
temperature remains constant, what must be
the prevailing air pressure at 5300 m?
Q74. A balloon indoors, where the
temperature is 27 °C, has a volume of 2.00
L. what will its volume be outdoors, where
the temperature is -23°C? (Assume no
change in gas pressure.)
Q75. At what temperature, in Kelvin and
degrees Celsius, should the balloon
described in Q74. be held to have a volume
of 2.25 L? (Assume a constant pressure.)
Q76. Calculate the volume occupied by
4.11 Kg of methane gas at STP?
Q77. The flask pictured contains O2, first at
STP and then at then at 100 C. what is the
pressure at 100 C?
Q78. What is the pressure exerted by 0.508
mol O2 in a 15.0 L container at 303 K?
Q79. What is the volume occupied by 16.0
g ethane gas (C2H6) at 720 torr and 18°C?
Q80. Calculate the molecular weight of a
gas if 0.550 g of the gas occupies 0.200 L at
0.968 atm and 289 K.
Q81. Calculate the molecular weight of a
liquid which, when vaporized at 100°C and
755 mmHg, yields 185 ml of vapor with a
mass of 0.523 g.
Q82. Calculate the density of methane gas
(CH4), in grams per liter, at 25 C and 0.978
atm.
Q83. Under what pressure must O2 be
maintained at 25°C to have a density of 1.50
g/L?
Q84. What volume of oxygen is required to
burn 0.556 L of propane, if both gases are
measured at the same temperature and
pressure?
C3H8 + 5O2
> 3CO2 + 4 H2O
Q85. In the chemical reaction used in
automotive air-bag safety systems, N2 is
produced by the high- temperature
decomposition of sodium azide, NaN3.
2NaN3
> 2 Na + 3N2
What volume of N2, measured at 25°C and
745 torr, is produced by the decomposition
of 62.5 g NaN3?
Q86. A 1.00L sample of dry air at 25°C
contains 0.0319 moles of N2, 0.00856 mole
of O2, 0.000381 mole of Ar, and 0.00002
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mole of CO2. Calculate the partial pressure
of N2 in the mixture.
Q87. The main components of dry air, by
volume are N2, 78.08%; O2, 20.95%; Ar,
0.93%; and CO2, 0.04%. What are the
partial pressures of each of the four gases in
a sample of air at 1.000 atm?
Q88. Oxygen is collected over water at
21°C. The total pressure inside the
collection jar is 741 torr. What is the
pressure due to the oxygen alone?
Q89. Hydrogen, produced by the following
reaction, is collected over water at 23°C and
742 torr barometric pressure.
2 Al + 6 HCl
> 2 AlCl3 + 3 H2.
What is the volume of that “wet” gas that
will be collected in the reaction of 1.50g Al
with excess HCl?
Q90. Calculate the relative rates of effusion
of hydrogen and helium under the same
conditions of temperature and pressure.
Q91. A sample of Ar escapes through a tiny
hole in 77.3 s. An unknown gas escape
under the same conditions in 97.6 s.
Calculate the molar mass of the unknown
gas?
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MISCELLANEOUS 2 (29)
Q92. Carry out the following conversions.
a. 722 torr to mmHg
b. 98.2 kPa to torr
c. 29.95 in Hg to torr
d. 768 torr to atm
Q93. Calculate the height of a column of
carbon tetrachloride, CCl4 that would exert
the same pressure as a column of mercury
that is 760 mm high. The density of CCl4 is
1.59 g/cm3 and that of Hg is 13.6 g/cm
3.
Q94. A diver reaches a depth of 30.0m.
What pressure, in atm, is exerted by water
at that depth?
Q95. A sample of air occupies 73.3 ml at
98.7 kPa and 0°C. What volume would the
air occupy at 4.02 atm and 0°C?
Q96. A sample of helium occupies 535 ml
at 988 torr and 25°C. if the sample is
transferred to a 1.05-L flask at 25 C, what
will be the gas pressure in the flask?
Q97. A sample of hydrogen occupies 692 L
at 602°C, if the pressure is held constant,
what volume will the gas occupy after
cooling to 23°C?
Q98. Solid carbon dioxide, called “dry ice”,
is useful in maintaining frozen foods
because it vaporizes to CO2 rather than
melting to a liquid. How many kilograms of
“dry ice” can be produced from 5.00 x 103
L CO2 measured at STP?
Q99. Aerosol containers often carry the
warning that they should not be heated.
Suppose such a container was filled with a
gas at 2.5 atm and 22°C and that the
container may rupture if the pressure
exceeds 8.0 atm. At what temperature is that
rupture likely to occur?
Q100. How many moles of nitrogen, N2, are
there in a sample occupies 35.0 L at a
pressure of 3.15 atm and a temperature of
852 K?
Q101. What is the temperature, in degrees
Celsius, at which 15.0 g O2 will exert a
pressure of 785 torr in a volume of 5.00 L?
Q102. How many grams are there in a
sample of N2 that occupies 525 ml at a
pressure of 546 torr and a temperature of
35°C?
Q103. Calculate the molar mass of a gas if
0.440 g occupies 179 ml at 741 mmHg and
86°C?
Q104. Calculate the molecular weight of a
liquid which, when vaporized at 98°C and
715 mmHg, yields 121 ml of vapor with a
mass of 0.471 g.
Q105. Diacetyl, a substance contributing to
the characteristic flavor and aroma of butter,
consists of 55.80% C, 7.03% H, and
37.17% O. In the gaseous state at 100°C
and 747 mmHg, a 0.3061 g sample occupies
a volume of 111 ml. Establish the molecular
formula of diacetyl.
Q106. Calculate the density of ethane gas
(C2H6), in grams per liter, at 15°C and 748
torr.
Q107. To what temperature must propane
gas (C3H8) at 785 torr be heated to have a
density of 1.51 g/L?
Q108. What volume of methane must
decompose to produce 10.0 L of hydrogen
in the following reaction, if the two gases
are compared at the same temperature and
pressure?
CH4
> C + 2H2
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Q109. The manufacture of quicklime CaO
for use in construction industry is
accomplished by decomposing limestone
CaCO3 by heating.
CaCO3
> CaO + CO2
How many liters of CO2 at 825°C and 754
torr are produced in the decomposition of
45.8 kg CaCO3?
Q110. How many kilograms of CaO are
formed in the decomposition of CaCO3 if
the volume of CO2 obtained is 1.25 x 104 L
at 825°C and 733 torr?
Q111. Calculate the partial pressure of each
of the other components of the air sample
containing 0.0319 moles of N2, 0.00856
mole of O2, 0.000381 mole of Ar, and
0.00002 mole of CO2. What is the total
pressure exerted by all the gases in the
sample?
Q112. What is the pressure exerted by a
mixture of 4.05 g N2, 3.15g H2, and 6.05g
He when confined to a 6.10 L container at
25°C?
Q113. A sample of expired air (air that has
been exhaled) is composed, by volume, of
the following main components: N2, 74.1%;
O2, 15.0%; H2O, 6.0%; Ar, 0.9%; and CO2,
4.0%. What are the partial pressures of each
of the five gases in the expired air at 37°C
and 1.000 atm?
Q114. A mixture of gases has methane at a
partial pressure of 505 torr, ethane at 201
torr, propane at 43 torr, and butane at 11.2
torr. Calculate the mole fraction of each
component.
Q115. What is the total volume of gas, in
liters, that will be obtained if 1.28g N2 is
collected over water at 21°C and a
barometric pressure of 696 torr?
Q116. Hydrogen gas is collected over water
at 18°C. The total pressure inside the
collection jar is set at the barometric
pressure of 738 torr. If the volume of the
gas is 246 ml, what mass of hydrogen is
collected? What is the mass of the wet gas?
Q117. A sample of KClO3 was decomposed
to potassium chloride and oxygen by
heating. The evolved O2 was collected over
water at 21°C and a barometric pressure of
746 mmHg. A 155 ml volume of the
gaseous mixture was obtained. What mass
of KClO3 was decomposed?
Q118. Calculate the relative rates of
effusion of N2 and A ruder the same
conditions of temperature and pressure.
Q119. A sample of N2 effuse from a tiny
opening in 57 s. an unknown gas escapes
under the same conditions in 83 s. calculate
the molar mass of the unknown gas.
Q120. A sample of O2 effuses from an
orifice in 123 s. how long should it take a
similar sample of methane, CH4, to effuse
under the same conditions?
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DESCRIPTIVE
QUESTIONS (18)
Q1. What is the nucleus? Describe the
nuclear atom.
Q2. When a light is emitted by an atom,
what change has occurred within an atom?
Q3. When a light is absorbed by an atom,
what change has occurred within an atom?
Q4. Which atom absorbs more energy: One
in which an electron moves from the second
energy level to the third level or an
otherwise identical atom in which an
electron moves from first to the third energy
level? Justify your answer.
Q5. Describe the quantum numbers and list
their possible values.
Q6. How many sublevels are there in an
energy level with each of the following
values of n?
a) n = 2 b) n = 3 c) n = 4
Q7. What is the geometric shape described
by a p-orbital?
Q8. What is the geometric shape described
by an s-orbital? How does a 2s orbital differ
from 1s orbital?
Q9. How many orbitals are there in of the
4f type?
Q10. Is there a 3d subshell in the hydrogen
atom? Explain.
Q11. What is the lowest numbered principal
shell in which p orbitals are found?
Q12. What is the lowest numbered principal
shell in which f orbitals are found?
Q13. If n = 5, what are the possible values
of l? If l = 3, what are the possible values of
m?
Q14. If n = 4, what are the possible values
of l? If l = 1, what are the possible values of
m?
Q15. Indicate, if each of the following is a
permissible set of quantum numbers. If the
set is not permissible, state why is it not
a) n = 2 l = 1 m = +1
b) n = 3 l = 3 m = -3
c) n = 3 l = 2 m = -2
d) n = 0 l = 0 m = 0
e) n = 3 l = 1 m = +2
f) n = 4 l = 3 m = -3
g) n = 3 l = 2 m = +2
h) n = 5 l = 0 m = 0
Q16. Consider the electronic structure of an
atom:
(a) What are the n, l and m quantum
numbers corresponding to the 3s orbital?
(b) List all the possible quantum number
values for an orbital in the 5f subshell.
(c) In what specific subshell, will an
electron having the quantum numbers n = 3,
l = 1 and m = -1 be found?
Q17. Consider the electronic structure of an
atom:
(a) What are the n, l and m quantum
numbers corresponding to the 3p orbital?
(b) List all the possible quantum number
values for an orbital in the 4d subshell.
(c) In what specific subshell, will an
electron having the quantum numbers n = 3,
l = 2 and m = 0 be found?
Q18. The greatest probability of finding an
electron in a small volume element of the 1s
orbital of hydrogen atom is at the nucleus.
Yet the most probable distance of the
electron from the nucleus is 52.9 pm. How
can you reconcile these two statements?
Q19. Show that if an electron in a Hydrogen
atom drops from the level n = 3 to n = 2,
followed by a drop from n = 2 to n = 1, the
total energy emitted is the same if the
electron had fallen directly from the level n
= 3 to n = 1.
Q20. Write down the electronic
classification of all the elements of the
modern periodic table.
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DESCRIPTIVE
QUESTIONS (7)
Q1. You are studying a sample of copper
(II) sulfate solution in a beaker on a ring
stand. The beaker is being heated by the
flame of a Bunsen burner. What is a logical
choice to describe as the system? What type
of a system is it? Describe the surrounding
for your choice of the system.
Q2. Can a system do work and absorb heat
at the same time? Can it do so while
maintain a constant internal energy?
Q3. Can a system do work and give off heat
at the same time? Can it do so while
maintain a constant internal energy?
Q4. How is enthalpy of a system, related to
its internal energy (E)?
Q5. Under what conditions, is the heat of
the reaction equals to the change in internal
energy in a reaction?
Q6. Under what conditions, is the heat of
the reaction equals to the change of enthalpy
in a reaction?
Q7. Upon heating under constant pressure,
solid calcium carbonate decomposes to solid
calcium oxide and carbon dioxide. In one
experiment, 17.8 KJ of heat is added to the
system to decompose 0.100 mole of CaCO3.
Is the reaction exothermic or endothermic?
What is the value of ∆H for the reaction of
one mole of CaCO3?
FIRST LAW OF
THERMODYNAMICS (4)
Q8. What is the change in internal energy
of a system that absorbs 455 J of heat and
does 325 J of work?
Q9. What is the change in internal energy
of a system that has 625 J of work done on it
and gives off 515 J of heat?
Q10. How much work, in joules, must be
involved in a process in which system gives
off 58 cal of heat, if the internal energy of
the system is remained to be unchanged?
Q11. If ∆E for a system is 217 J in a process
in which the system absorbs 185 cal of heat.
How much work in joules, is involved?
ENTHALPY CHNAGES (6)
Q12. At high temperatures water is
decomposed to give hydrogen and oxygen.
2 H2O ───> 2 H2 + O2
Decomposition of 10.0 g H2O in a isobaric
process requires 134 kJ of heat to be
absorbed by the system. Determine if the
reaction is an exothermic or endothermic?
What is the value of q for the reaction, per
mole of water? Is the value of q equals to ∆E
or ∆H? Explain.
Q13. Combustion of 0.144 g of sucrose
(table sugar, C12H22O11) results in release of
2.38 kJ of heat.
C12H22O11 + 12 O2 ───> 12 CO2 + 11 H2O
Is the reaction endothermic or exothermic?
What is the value of q for the reaction, per
mole of sucrose? How would you expect the
values of ∆E and ∆H to compare for this
reaction? Explain
Q14. When 0.0500 mole of solid CaCO3 is
heated in air, it decomposes to solid CaO and
CO2 gas. 8.9 kJ of heat is absorbed. Write
the chemical equation for the decomposition
of one mole of CaCO3 and the value of ∆H.
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Q15. When 0.200 mole of ethane gas is
burnt in excess oxygen, 312 kJ of heat is
evolved. Write the chemical equation for the
decomposition of one mole of CaCO3 and
the value of ∆H.
Q16. Given the reaction:
3 Fe2O3 + CO ───> 2 Fe3O4 + CO2
∆H°= -- 46kJ
Calculate ∆H for the following reactions:
a) Fe2O3 + �
� CO ───>
�
� Fe3O4 +
�
� CO2
b) Fe3O4 + �
� CO2 ───>
�
� Fe2O3 +
�
� CO
Q17. Given the reaction:
2 �a2O2 + 2 H2O ───> 4 �aOH + O2
∆H°= --109kJ
Calculate ∆H for the following reactions:
a) �a2O2 + H2O ───> 2 �aOH + ½ O2
b) �aOH + �
� O2 ───> ½ �a2O2 + ½ H2O
CALCULATION OF HEATS
REACTION (4)
Q18. Calcium oxide (lime) reacts with water
to form calcium hydroxide (slaked lime).
CaO + H2O ───> Ca(OH)2
∆H°= -- 65.2 kJ
How much heat, in joules is evolved when
0.333 mole Ca(OH)2 is formed?
Q19. Calcium carbide can be made by
heating calcium oxide with carbon.
CaO + 3C ───> CaC2 + CO
∆H°= + 464.8 kJ
How much heat, in joules, is absorbed in a
reaction in which 2.79 mole Carbon is
consumed under these conditions?
Q20. Iron (III) oxide is reduced to iron metal
by reaction with carbon monoxide.
Fe2O3 + 3 CO ───> 2 Fe + 3CO2
∆H°= -- 24.8 kJ
How many kilograms of CO are consumed
when 429 J of heat is released under these
conditions?
Q21. Calcium Carbide reacts with water to
form acetylene (C2H5) a gas used as a fuel in
welding.
CaC2 + 2 H2O ───> C2H2 + Ca(OH)2
∆H°= -- 128.0 kJ
How many kilograms of CaC2 are
consumed in a reaction 3.64 x 104 kJ of heat
under these conditions?
MEASUREMENT OF HEAT (10)
Q22. Calculate the heat capacity of a piece
of iron if a temperature rise from 18°C to
45°C requires 112 J of heat.
Q23. Calculate the heat capacity of a sample
of radiator coolant if temperature rise from -
5°C to 142°C requires 932 J of heat.
Q24. How much heat in kilojoules, is
required to raise the temperature of:
(a) 20 g of water from 20°C to 96°C
(b) 120 g ethanol from -10.5°C to 44.5°C
Q25. How much heat in kilojoules, is
released when the temperature of:
(a) 47 g of water drops from 45.4°C to 10°C
(b) 209 g iron drops from 400°C to 22.6°C
Q26. A 48.7 g block of lead initially at 27°C
absorbs 93.5 J of heat. What is the final
temperature of lead? (Specific Heat of Lead
is 0.128 J/g°C)
Q27. A 454 g iron block initially at 16°C
absorbs 63.9 kJ of heat. What is the final
temperature of iron? (Specific Heat of Iron is
0.449 J/g°C)
Q28. A 10.25 g sample of a metal alloy wire
us heated to 99.10°C. It is then quickly
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dropped into 20 g of water in a calorimeter.
The water temperature rises from 18.51°C to
22.03°C. Calculate the specific heat of alloy.
Q29. A 2.05 g sample of a metal alloy wire
us heated to 98.88°C. It is then quickly
dropped into 28 g of water in a calorimeter.
The water temperature rises from 19.73°C to
21.23°C. Calculate the specific heat of alloy.
Q30. A 1.35 kg piece of iron is quickly
dropped into 0.817 kg of water, and the
water temperature rises from 23.3°C to
39.6°C. What must have been the initial
temperature?
Q31. A piece of stainless steel is taken from
an oven at 178°C and quickly immersed in
225 ml of water at 25.9°C. The water
temperature rises to 42.4°C. What is the
mass of the piece of steel? (Specific Heat of
Stainless Steel is 0.5 J/g°C)
MISCELLANEOUS 1 (23)
Q32. A gas does 135 J of work while
expanding, and at the same time it absorbs
156 J of heat. What is the change in internal
energy (E)?
Q33. Use the following equation:
S8 + 4 O2 + 8 Cl2 ───> 8 SOCl2
∆H= -- 1694 kJ
to calculate ∆H for the reaction: �
� S8 + ½ O2 + Cl2 ───> SOCl2
Q34. Given the equation:
H2 + I2 ───> 2HI
∆H= + 52.96 kJ
Calculate ∆H for the reaction:
HI ───> ½ H2 + ½ I2
Q35. What is the enthalpy change associated
with the formation of 5.67 mole HCL in the
reaction?
H2 + Cl2 ───> 2HCl
∆H= -- 184.6 kJ
Q36. Calculate the heat capacity of an
aluminum block if a temperature rise from
22°C to 145°C requires the absorption of 629
J of heat.
Q37. How much heat, in joules and
kilocalories, does it take to raise the
temperature of 225 g of water from 25°C to
100°C?
Q38. How many kilograms of water can be
heated from 5.5°C to 55°C by 9.09 x 1010
J
of heat?
Q39. What will be the final temperature if 25
J of heat is removed from a 5 g silver ring
that is initially at 37°C? (Specific Heat of
Stainless Steel is 0.235 J/g°C)
Q40. A 15.5 g sample of a metal alloy is
heated to 98.9°C and then dropped into 25g
of water in a calorimeter. The temperature of
the water rises from 22.5°C to 25.7°C.
Calculate the specific heat of the alloy.
MISCELLANEOUS 2 (29)
Q41. In a process in which 89 J of work is
done on a system, 567 J of heat is given off.
What is ∆E of the system?
Q42. Use the equation:
3 O2 ───> 2 O3
∆H= + 285.4 kJ
To calculate ∆H for the reaction: �
� O2 ───> O3
Q43. From the equation:
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2 Ag2S + 2 H2O ───> 4Ag + 2 H2S + O2
∆H= + 595.5 kJ
Calculate ∆H for the reaction:
Ag + ½ H2S + ½ O2 ───>½ Ag2S + ½ H2O
Q44. What is the enthalpy change when 12.8
H2 reacts with excess Cl2 to form HCl?
H2 + Cl2 ───> 2HCl
∆H= -- 184.6 kJ
Q45. What volume of CH4 measured at 25°C
and 745 torr, must be burnt in excess oxygen
to release 1 x 10 kJ of heat to the
surroundings?
CH4 + 2 O2 ───> CO2 + 2H2O
∆H= -- 890.3 kJ
Q46. Calculate the heat capacity of a sample
of break fluid if a temperature rise from
15°C to 100°C requires the absorption of 911
J of heat.
Q47. How much heat, in calories and
kilocalories, does it take to raise the
temperature of 814 g of water from 18°C to
100°C?
Q48. A 454 g of lead is at an initial
temperature of 22.5°C. What will be the
temperature of the lead, after 4.22 kJ of heat
is added? (Specific Heat of Lead is 0.13
J/g°C)
Q49. How many gram of copper can be
heated from 22.5°C to 35°C by a quantity of
heat sufficient to raise the temperature of 145
g of H2O through the same interval?
(Specific Heat of Copper is 0.385 J/g°C)
Q50. A 23.9 g sample of iridium is heated to
89.7°C and then dropped into 20g of water in
a calorimeter. The temperature of the water
rises from 20.1 to 22.6°C. Calculate the
specific heat of iridium.
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WORKSHEET
HA�DOUT 2
MISCELLA�EOUS 1
Q51. 146 amu
Q52. 132 amu
Q53. 5.75 g
Q54. 5.11 moles
Q55. 1.74x1022
ions
Q56. 3.8 x 10-23
g
Q57. N= 40% H= 14.2% O=45.71%
Q58. 16.22 g
Q59. C6H6O
Q60. C4H10O3
Q61. C6H6O2
Q62. C=53.3%, H= 11.1% O=35.6%,
C2H5O C4H10O2
Q63. 0.525 moles
Q64. 340 g
Q65. 52 g solution
Q66. 124.02 g 74g
Q67. 202.13 g
Q68. 0.333 M
Q69. 133 g
Q70. 14.8 M
Q71. 50 ml
Q72. 0.05040 M
Q73. 10.25 ml
WORKSHEET
HA�DOUT 2
MISCELLA�EOUS 2
Q74. 244g 129g 258g 211g
Q75. 295g 297g 87g 342g
Q76. 0.06
moles
9.3x10-4
moles
2.8x104
moles
0.01 moles
Q77. 999g 0.75g 7.35x10-3
g 134.2g
Q78. 9.2x1022
atoms
2.5x1020
mol
1.92x1023
mol
1.17x1025
atoms
Q79. 6.6x10-23
g 3.5x10-22
g 2.5x10-22
g 7.3x10-23
g
Q80. N=21.2% H= 6%, S=24.2% O=48.5%
C=20% O=26.6% N=46.6%, H=6.6%),
Urea
Q81. 1370mg
Q82. C5H10NO2
Q83. C2H2NO
Q84. C2H4 C6H12 C5H10
Q85. C=80.2% H=9.4% O=10.4% C21H30O2
Q86. 1.587 moles 304.8
moles
6x10-3
moles
Q87. 21.12g
Q88. 0.96g
Q89. 774 ml
Q90. 4.75g
Q91. 25.15g
Q92. 269.4g
Q93. 9M 1.25M 0.27M 0.024M
1.09M
Q94. 672g 5.6g 0.056g 4.62 g
Q95. 23.5M
Q96. 466ml
Q97. 0.172M
Q98. 375ml