chem ii practice test chapter 5.docx

Chem II Practice Test

____ 1) At what velocity (m/s) must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J?A) 1.00 D) 1.00 103

B) 100 102 E) 50.0C) 10.0

____ 2) Objects can possess energy as __________.

(a) endothermic energy(b) potential energy(c) kinetic energy

A) a only D) a and cB) b only E) b and cC) c only

____ 3) The internal energy of a system is always increased by __________.A) adding heat to the system D) adding heat to the system and having

the system do work on the surroundings

B) having the system do work on the surroundings

E) a volume compression

C) withdrawing heat from the system

____ 4) The internal energy of a system __________.A) is the sum of the kinetic energy of all

of its componentsD) is the sum of the potential and kinetic

energies of the componentsB) is the sum of the rotational,

vibrational, and translational energies of all of its components

E) none of the above

C) refers only to the energies of the nuclei of the atoms of the component molecules

____ 5) Which one of the following conditions would always result in an increase in the internal energy of a system?A) The system loses heat and does work

on the surroundings.D) The system gains heat and has work

done on it by the surroundings.B) The system gains heat and does work

on the surroundings.E) None of the above is correct.

C) The system loses heat and has work done on it by the surroundings.

____ 6) The value of ÄE for a system that performs 111 kJ of work on its surroundings and gains 89 kJ of heat is __________ kJ.A) -111 D) -22B) -200 E) 22C) 200

____ 7) The value of ÄE for a system that performs 13 kJ of work on its surroundings and loses 9 kJ of heat is __________ kJ.A) 22 D) 4B) -22 E) -13C) -4

____ 8) When a system __________, E is always negative.A) absorbs heat and does work D) gives off heat and has work done on itB) gives off heat and does work E) none of the above is always negative.C) absorbs heat and has work done on it

____ 9) Which one of the following is an endothermic process?A) ice melting D) Hydrochloric acid and barium

hydroxide are mixed at 25 °C: the temperature increases.

B) water freezing E) Both A and CC) boiling soup

____ 10) Which one of the following is an exothermic process?A) ice melting D) condensation of water vaporB) water evaporating E) Ammonium thiocyanate and barium

hydroxide are mixed at 25 °C: the temperature drops.

C) boiling soup

____ 11) Of the following, which one is a state function?A) H D) heatB) q E) none of the aboveC) w

____ 12) Which of the following is a statement of the first law of thermodynamics?A)

Ek = mv2

D) Energy lost by the system must be gained by the surroundings.

B) A negative ÄH corresponds to an exothermic process.

E) 1 cal = 4.184 J (exactly)

C) E = Efinal – Einitial

____ 13) The internal energy can be increased by __________.

(a) transferring heat from the surroundings to the system(b) transferring heat from the system to the surroundings (c) doing work on the system

A) a only D) a and cB) b only E) b and cC) c only

____ 14) A __________ H corresponds to an __________ process.A) negative, endothermic D) zero, exothermicB) negative, exothermic E) zero, endothermicC) positive, exothermic

____ 15) A __________ H corresponds to an __________ process.A) negative, endothermic D) zero, exothermicB) positive, exothermic E) zero, endothermicC) positive, endothermic

____ 16) H for an endothermic process is __________ while H for an exothermic process is __________.A) zero, positive D) negative, positiveB) zero, negative E) positive, negativeC) positive, zero

____ 17) For a given process at constant pressure, H is negative. This means that the process is __________.A) endothermic D) a state functionB) equithermic E) energyC) exothermic

____ 18) Which one of the following statements is true?A) Enthalpy is an intensive property. D) H is the value of q measured under

conditions of constant volume.B) The enthalpy change for a reaction is

independent of the state of the reactants and products.

E) The enthalpy change of a reaction is the reciprocal of the ÄH of the reverse reaction.

C) Enthalpy is a state function.

____ 19) Which of the following statements is false?A) Internal energy is a state function. D) The enthalpy change for a reaction

depends on the state of the reactants and products.

B) Enthalpy is an intensive property. E) The enthalpy of a reaction is equal to

the heat of the reaction.C) The enthalpy change for a reaction is

equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction.

____ 20) A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ H at constant pressure.A) endothermic, positive D) exothermic, positiveB) endothermic, negative E) exothermic, neutralC) exothermic, negative

____ 21) A chemical reaction that releases heat to the surroundings is said to be __________ and has a __________ H at constant pressure.A) endothermic, positive D) exothermic, positiveB) endothermic, negative E) exothermic, neutralC) exothermic, negative

____ 22) The reaction

4Al (s) + 3O2 (g) 2 Al2O3 (s) H° = -3351 kJis __________, and therefore heat is __________ by the reaction.A) endothermic, released D) exothermic, absorbedB) endothermic, absorbed E) thermoneutral, neither released nor

absorbedC) exothermic, released

____ 23) Under what condition(s) is the enthalpy change of a process equal to the amount of heat transferred into or out of the system?

(a) temperature is constant(b) pressure is constant(c) volume is constant

A) a only D) a and bB) b only E) b and cC) c only

____ 24) The units of of heat capacity are __________.A) K/J or °C/J D) J/molB) J/K or J/°C E) g-K/J or g-°C/JC) J/g-K or J/g-°C

____ 25) The units of of specific heat are __________.A) K/J or °C/J D) J/mol

B) J/K or J/°C E) g-K/J or g-°C/JC) J/g-K or J/g-°C

____ 26) The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1 °F. There are __________ joules in one Btu. 1 lb = 453.59 g; °C = (5/9)(°F - 32°); specific heat of H2O (l) = 4.184 J/g-K.A) 3415 D) 5.120 10-3

B) 60.29 E) Additional information is needed to complete the calculation.

C) 1054

____ 27) A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams) of the sample?A) 3.7 D) 410B) 5.0 E) 5.0 103

C) 7.5

____ 28) The temperature of a 12.58 g sample of calcium carbonate [CaCO3 (s)] increases from 23.6 °C to 38.2 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed?A) 0.82 D) 410B) 5.0 E) 151C) 7.5

____ 29) An 8.29 g sample of calcium carbonate [CaCO3 (s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. What is the specific heat of calcium carbonate?A) .63 D) 2.2B) .82 E) 4.2C) 1.1

____ 30) A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 °C to 28.5 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample?A) 4.3 D) 1100B) 11 E) 1.1 103

C) 21

____ 31) The temperature of a 35.2 g sample of iron increases from 23.7 °C to 29.5 °C. If the specific heat of iron is 0.450 J/g-K, how many joules of heat are absorbed?A) 4.3 D) 1100

B) 92 E) 1.1 103

C) 0.450

____ 32) A 22.44 g sample of iron absorbs 180.8 J of heat, upon which the temperature of the sample increases from 21.1 °C to 39.0 °C. What is the specific heat of iron?A) 0.140 D) 0.840B) 0.450 E) 0.900C) 0.820

____ 33) Which of the following is a statement of Hess's law?A) If a reaction is carried out in a series of

steps, the H for the reaction will equal the sum of the enthalpy changes for the individual steps.

D) The H for a process in the forward direction is equal to the H for the process in the reverse direction.

B) If a reaction is carried out in a series of steps, the H for the reaction will equal the product of the enthalpy changes for the individual steps.

E) The H of a reaction depends on the physical states of the reactants and products.

C) The H for a process in the forward direction is equal in magnitude and opposite in sign to the ÄH for the process in the reverse direction.

____ 34) For which one of the following reactions is H°rxn equal to the heat of formation of the product?A) N2 (g) + 3H2 (g) 2NH3 (g) D) P (g) + 4H (g) + Br (g) PH4Br (l)B) (1/2) N2 (g) + O2 (g) NO2 (g) E) 12C (g) + 11H2 (g) + 11O (g)

C6H22O11 (g)C) 6C (s) + 6H (g) C6H6 (l)

____ 35) Of the following, Hf° is not zero for __________.A) O2 (g) D) F2 (s)B) C (graphite) E) Cl2 (g)C) N2 (g)

____ 36) Of the following, Hf° is not zero for __________.A) Sc (g) D) Br2 (l)B) Si (s) E) Ca (s)C) P4 (s, white)

____ 37) Consider the following two reactions:

A 2B H°rxn = 456.7 kJ/molA C H°rxn = -22.1kJ/mol

Determine the enthalpy change for the process:

2B CA) -478.8 kJ/mol D) 478.8 kJ/molB) -434.6 kJ/mol E) More information is needed to solve

the problem.C) 434.6 kJ/mol

____ 38) In the reaction below, Hf° is zero for __________.Ni (s) + 2CO (g) + 2PF3 (g) Ni(CO)2 (PF3)2 (l)

A) Ni (s) D) Ni(CO)2(PF3)2 (l)B) CO (g) E) both CO (g) and PF3 (g)C) PF3 (g)

____ 39) For the species in the reaction below, Hf° is zero for __________.2Co (s) + H2 (g) + 8PF3 (g) 2HCo(PF3)4 (l)

A) Co (s) D) HCo(PF3)4 (l)B) H2 (g) E) both Co(s) and H2 (g)C) PF3 (g)

____ 40) For which one of the following equations is H°rxn equal to Hf° for the product?A) Xe (g) + 2 F2 (g) XeF4 (g) D) 2CO (g) + O2 (g) 2CO2 (g)B) CH4 (g) + 2 Cl2 (g) CH2 Cl2 (l) +

2HCl (g)E) C (diamond) + O2 (g) CO2 (g)

C) N2 (g) + O3 (g) N2O3 (g)

____ 41) For which one of the following reactions is the value of H°rxn equal to Hf° for the product?A) 2Ca (s) + O2 (g) 2CaO (s) D) 3Mg (s) + N2 (g) Mg3N2 (s)B) C2H2 (g) + H2 (g) C2H4 (g) E) C (diamond) + O2 (g) CO2 (g)C) 2C (graphite) + O2 (g) 2CO (g)

____ 42) For which one of the following reactions is the value of H°rxn equal to Hf° for the product?A) 2 C (s, graphite) + 2 H2 (g) C2H4 (g) D) 2 H2 (g) + O2 (g) 2 H2O (g)B) N2 (g) + O2 (g) 2 NO (g) E) H2O (l) + 1/2 O2 (g) H2O2 (l)C) 2 H2 (g) + O2 (g) 2 H2O (l)

____ 43) For which one of the following reactions is the value of H°rxn equal to Hf° for the product?A) H2O (l) + 1/2 O2 (g) H2 O2 (l) D) 2H2 (g) + O2 (g) 2H2O (g)B) N2 (g) + O2 (g) 2NO (g) E) none of the aboveC) 2H2 (g) + O2 (g) 2H2O (l)

____ 44) For which one of the following reactions is the value of H°rxn equal to Hf° for the product?A) H2 (g) + 1/2 O2 (g) H2O (l) D) 1/2 N2 (g) + O2 (g) NO2 (g)

B) H2 (g) + O2 (g) H2O2 (l) E) all of the aboveC) 2 C (s, graphite) + 2 H2 (g) C2H4 (g)

____ 45) With reference to enthalpy changes, the term standard conditions means __________.(a) P = 1 atm (b) some common temperature, usually 298 K(c) V = 1 L

A) a only D) a and cB) b only E) a and bC) c only

____ 46) The energy released by combustion of 1 g of a substance is called the __________ of the substance.A) specific heat D) heat capacityB) fuel value E) enthalpyC) nutritional calorie content

____ 47) Fuel values of hydrocarbons increase as the H/C atomic ratio increases. Which of the following compounds has the highest fuel value?A) C2H6 D) CH4

B) C2H4 E) C6H6

C) C2H2

____ 48) Of the substances below, the highest fuel value is obtained from __________.A) charcoal D) hydrogenB) bituminous coal E) woodC) natural gas

____ 49) Which one of the choices below is not considered a fossil fuel?A) anthracite coal D) hydrogenB) crude oil E) petroleumC) natural gas

____ 50) The most abundant fossil fuel is __________.A) natural gas D) uraniumB) petroleum E) hydrogenC) coal

____ 51) Calculate the kinetic energy in J of an electron moving at 6.00 106 m/s. The mass of an electron is 9.11 10-28 g.A) 4.98 10-48 D) 2.49 10-48

B) 3.28 10-14 E) 6.56 10-14

C) 1.64 10-17

____ 52) Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph. (1 mile = 1.6093 km, 1 lb = 453.59 g)A) 1.2 104 D) 3.2 106

B) 2.9 105 E) 3.2 10-6

C) 5.9 105

____ 53) Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. (1 mile = 1.6093 km, 1 lb = 453.59 g)A) 5.5 x 105 D) 2.2 106

B) 5.5 10-5 E) 2.2 10-6

C) 1.1 106

____ 54) The kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s is __________ J.A) 1.2 103 D) 1.3 102

B) 66 E) 7.3C) 2.4 103

____ 55) The kinetic energy of a 10.3 g golf ball traveling at 48.0 m/s is __________ J.A) 1.20 103 D) 1.3 102

B) 66 E) 23.7C) 11.9

____ 56) Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg) traveling at 12.0 mile/hr (5.36 m/s).A) 1.96 103 D) 183B) 365 E) 68.1C) 978

____ 57) Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.A) 3.60 106 D) 12.0B) 1.20 104 E) 80.0C) 3.60 103

____ 58) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ J.A) 1900 D) 1.43 10-3

B) 77.8 E) 6.00C) 145

____ 59) The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ kcal.A) 1.43 10-3 D) 454

B) 6.00 E) 0.0251C) 1900

____ 60) A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W) = 1 J/sec]A) 2.40 103 D) 2.10 103

B) 8.64 103 E) 8.64 106

C) 4.17

____ 61) The E of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is __________ J.A) 16.6 D) -16.6B) 12.4 E) -8.2C) 4.2

____ 62) The E of a system that absorbs 12.4 J of heat and does 4.2 J of work on the surroundings is __________ J.A) 16.6 D) -16.6B) 12.4 E) 8.2C) 4.2

____ 63) The change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.A) 10,155 D) -10,155B) 5,155 E) 1.91 107

C) -5,155

____ 64) The change in the internal energy of a system that releases 2,500 J of heat and that does 7,655 J of work on the surroundings is __________ J.A) -10,155 D) 10,155B) -5,155 E) 5,155C) -1.91 107

____ 65) The value of ÄH° for the reaction below is -72 kJ. __________ kJ of heat are released when 80.9 grams of HBr is formed in this reaction.

H2 (g) + Br2 (g) 2HBr (g)A) 144 D) 36B) 72 E) -72C) 0.44

____ 66) The value of ÄH° for the reaction below is -126 kJ. __________ kj are released when 2.00 mol of NaOH is formed in the reaction?

2 Na2O2 (s) + 2 H2O (l) 4NaOH (s) + O2 (g)A) 252 D) 7.8B) 63 E) -126C) 3.9

____ 67) The value of H° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is __________ kJ.

2S (s) + 3O2 (g) 2SO3 (g)A) 23 D) 12B) -23 E) -790C) -12

____ 68) The value of ÄH° for the reaction below is -6535 kJ. __________ kJ of heat are released in the combustion of 16.0 g of C6H6 (l)?

2 C6H6 (l) + 15 O2 (g) 12CO2 (g) + 6 H2O (l)A) 1.34 103 D) 2.68 103

B) 5.23 104 E) -6535C) 669

____ 69) The value of H° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 38.5 g of O2 (g) reacts with excess CO.

2CO (g) + O2 (g) 2CO2 (g)A) 2.65 103 D) 65.7B) 482 E) 210.C) 580.

____ 70) The value of H° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed.

CH4 (g) + 3 Cl2 (g) CHCl3 (l) + 3HCl (g)A) 177 D) 211B) 2.57 103 E) -336C) 70.7

____ 71) The value of H° for the reaction below is -186 kJ. Calculate the heat (kJ) released from the reaction of 25 g of Cl2.

H2 (g) + Cl2 (g) 2HCl (g)A) 66 D) 47B) 5.3 102 E) -186

C) 33

____ 72) The enthalpy change for the following reaction is -483.6 kJ:

2 H2 (g) + O2 (g) 2 H2O (g)

Therefore, the enthalpy change for the following reaction is __________ kJ:4 H2 (g) + 2 O2 (g) 4 H2O (g)

A) -483.6 D) 483.6B) -967.2 E) 967.2C) 2.34 105

____ 73) The value of H° for the reaction below is +128.1 kJ:

CH3OH (l) CO (g) + 2 H2 (g)How many kJ of heat are consumed when 15.5 g of CH3OH (l) decomposes as shown in the equation?A) 0.48 D) 32B) 62.0 E) 8.3C) 1.3 102


CH3OH (l) CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.10 g of H2 (g) is formed as shown in the equation?A) 162 D) 653B) 62.0 E) 326C) 128


CH3OH (l) CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation?A) 0.182 D) 23.3B) 162 E) 62.0C) 8.31


CH3OH (l) CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.75 g of CO (g) is formed as shown in the equation?

A) 23.3 D) 162B) 62.0 E) 8.3C) 26.3

____ 77) The value of ÄH° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) 2BaO (s)

How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?A) 96.3 D) 23.2B) 26.3 E) 193C) 46.4

____ 78) The value of H° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) 2BaO (s)

How many kJ of heat are released when 5.75 g of BaO (s) is produced?A) 56.9 D) 193B) 23.2 E) 96.3C) 20.8

____ 79) The value of H° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) 2BaO (s)

How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?A) 20.8 D) 70.3B) 63.5 E) 35.1C) 114

____ 80) The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.A) 88.0 D) 6.88 103

B) 1.13 E) -88.0C) 4.89

____ 81) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?A) 2.0 D) 29B) -0.13 E) 0.13

C) 5.8 10-4

____ 82) The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.A) 7.8 D) 0.13B) 1.9 E) -29C) 29

____ 83) The specific heat of bromine liquid is 0.226 J/g K. The molar heat capacity (in J/mol-K) of bromine liquid is __________.A) 707 D) 9.05B) 36.1 E) 0.226C) 18.1

____ 84) The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.A) 5.20 D) 32.4B) 16.2 E) 10.4C) 300

____ 85) ÄH for the reaction

IF5 (g) IF3 (g) + F2 (g)

is __________ kJ, give the data below.

IF (g) + F2 (g) IF3 (g) H = -390 kJ

IF (g) + 2 F2 (g) IF5 (g) H = -745 kJA) +355 D) +35B) -1135 E) -35C) +1135

____ 86) Given the following reactionsFe2O3 (s) + 3CO (s) ? 2Fe (s) + 3CO2 (g) H = -28.0 kJ

3Fe (s) + 4CO2 (s) ? 4CO (g) + Fe3O4 (s) H = +12.5 kJ

the enthalpy of the reaction of Fe2O3 with CO

3 Fe2O3 (s) + CO (g) ? CO2 (g) + 2 Fe3O4 (s)

is __________ kJ.

A) -59.0 D) -109B) 40.5 E) +109C) -15.5

____ 87) Given the following reactions

N2 (g) + 2 O2 (g) 2NO2 (g) H = 66.4 kJ

2NO (g) + O2 (g) 2NO2 (g) H = -114.2 kJ

the enthalpy of the reaction of the nitrogen to produce nitric oxide

N2 (g) + O2 (g) 2NO (g)

is __________ kJ.A) 180.6 D) 90.3B) -47.8 E) -180.6C) 47.8

____ 88) Given the following reactions(1) 2NO N2 + O2 H = -180 kJ (2) 2NO + O2 2NO2 H = -112 kJ

the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide

N2 + 2O2 2NO2

is __________ kJ.A) 68 D) 292B) -68 E) -146C) -292

____ 89) Given the following reactions:2S (s) + 3O2 (g) 2SO3 (g) H = -790 kJ S (s) + O2 (g) SO2 (g) H = -297 kJ

the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide

2SO2 (g) + O2 (g) 2SO3 (g)

is __________ kJ.A) 196 D) -1384B) -196 E) -543C) 1087


CaCO3 (s) CaO (s) + CO2 (g) H = 178.1 kJC (s, graphite) + O2 (g) CO2 (g) H = -393.5 kJ

the enthalpy of the reaction

CaCO3 (s) CaO (s) + C (s, graphite) + O2 (g)

is __________ kJ.A) 215.4 D) -571.6B) 571.6 E) 7.01 104

C) -215.4


H2O (l) H2O (g) H = 44.01 kJ2 H2 (g) + O2 (g) 2 H2O (g) H = -483.64 kJ

the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen

2 H2O (l) 2 H2 (g) + O2 (g)

is __________ kJ.A) -395.62 D) 571.66B) -527.65 E) 527.65C) 439.63


N2 (g) + O2 (g) 2NO (g) H = +180.7 kJ2 N2O (g) O2 (g) + 2N2 (g) H = -113.1 kJ

the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen2 N2O (g) O2 (g) + 2N2 (g)

is __________ kJ.A) 67.6 D) -293.8B) -67.6 E) 45.5C) 293.8

____ 93) Given the following reactionsN2 (g) + O2 (g) 2NO (g) H = +180.7 kJ2 N2O (g) O2 (g) + 2N2 (g) H = -113.1 kJ

the enthalpy of reaction for4NO (g) 2NO2 (g) + N2 (g)

is __________ kJ.

A) 67.6 D) -45.5B) 45.5 E) 293.8C) -293.8

____ 94) Given the following reactionsN2 (g) + O2 (g) 2NO (g) H = +180.7 kJ2 N2O (g) O2 (g) + 2N2 (g) H = -163.2 kJ

the enthalpy of reaction for2 N2O (g) 2NO (g) + N2 (g)

is __________ kJ.A) 145.7 D) 17.5B) 343.9 E) -145.7C) -343.9

____ 95) The value of H° for the reaction below is -186 kJ.

H2 (g) + Cl2 (g) 2HCl (g)

The value of Hf° for HCl (g) is __________ kJ/mol.A) -3.72 102 D) -186B) -1.27 102 E) +186C) -93.0

____ 96) The value of H° for the following reaction is -3351 kJ:

2Al (s) + 3O2 (g) 2 Al2O3 (s)

The value of Hf ° for Al2O3 (s) is __________ kJ.A) -3351 D) -16.43B) -1676 E) +3351C) -32.86

____ 97) Given the data in the table below, H°rxn for the reaction

Ca(OH)2 + 2 H3AsO4 Ca(H2AsO4)2 + 2 H2O

is __________ kJ.

A) -744.9 D) -130.4B) -4519 E) -76.4C) -4219


4NH3 (g) + 5 O2 (g) 4NO (g) + 6 H2O (l)

is __________ kJ.

A) -1172 D) -1892B) -150 E) The Hf ° of O2 (g) is needed for the

calculation.C) -1540


C2H5OH (l) + O2 (g) ? CH3CO2H (l) + H2O (l)

is __________ kJ.

A) -79.0 D) -492.6B) -1048.0 E) The value of Hf° of O2 (g) is required

for the calculation.C) -476.4

____ 100) Given the data in the table below, ÄH°rxn for the reaction

3NO2 (g) + H2O (l) 2HNO3 (aq) + NO (g)

is __________ kJ.

A) 64 D) -508B) 140 E) -64C) -140


IF5 (g) + F2 (g) IF7 (g)

is __________ kJ.

A) 1801 D) -121B) -1801 E) -101C) 121

____ 102) Given the data in the table below, H° for the reaction2CO (g) + O2 (g) 2CO2 (g)

is __________ kJ.

A) -566.4 D) -677.0B) -283.2 E) The H°f of O2 (g) is needed for the

calculation.C) 283.2

____ 103) The value of H° for the following reaction is 177.8 kJ. The value of Hf° for CaO(s) is __________ kJ/mol.

CaCO3 (s) CaO (s) + CO2 (g)

A) -1600 D) 813.4B) -813.4 E) 177.8C) -635.5


2 AglS (s) + O2 (g) 2 Ag2O (s) + 2S (s)

is __________ kJ.

A) -1.6 D) +3.2B) +1.6 E) The H°f of S (s) and of O2 (g) are

needed for the calculation.C) -3.2


Ag2O (s) + H2S (g) Ag2S (s) + H2O (l)

is __________ kJ.

A) -267 D) -308B) -370 E) More data are needed to complete the

calculation.C) -202


2SO2 (g) + O2 (g) 2SO3 (g)

is __________ kJ.

A) -99 D) 198B) 99 E) The H°f of O2 (g) is needed for the

calculation.C) -198

____ 107) Given the data in the table below, H°rxn for the reactionSO3 (g) + H2O (l) H2SO4 (l)

is __________ kJ.

A) -132 D) -704B) 1496 E) -2.16 103

C) 704


3 Cl2 (g) + PH3 (g) PCl3 (g) + 3 HCl (g)

is __________ kJ.

A) -385.77 D) 385.77B) -570.37 E) The H°f of Cl2 (g) is needed for the



PCl3 (g) + 3 HCl (g) 3 Cl2 (g) + PH3 (g)

is __________ kJ.

A) -570.37 D) 385.77B) -385.77 E) The ÄH°f of Cl2 (g) is needed for the


____ 110) Given the data in the table below and H°rxn for the reaction

SO2Cl2 (g) + 2 H2O (l) H2SO4 (l) + 2HCl (g) H° = -62 kJ

H°f of HCl (g) is __________ kJ/mol.

A) -184 D) 30B) 60 E) Insufficient data are given.C) -92

____ 111) A 25.5-g piece of cheddar cheese contains 37% fat, 28% protein, and 4% carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value for this piece of cheese is __________ kJ.A) 450 D) 99B) 330 E) 260C) 790

____ 112) The average fuel value of sugars is 17 kJ/g. A 2.0 L pitcher of sweetened Kool-Aid contains 400 g of sugar. What is the fuel value (in kJ) of a 500 mL serving of Kool-Aid? (Assume that the sugar is the only fuel source.)A) 4.2 104 D) 1.7 102

B) 1.7 103 E) 17C) 1.7 106

____ 113) A meal containing a burger, fries, and a milkshake contains 53.0 grams of fat, 38.0 grams of protein, and 152 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If swimming typically burns 1100.0 kJ/hour, __________ minutes of swimming are required to completely burn off the meal.A) 4.78 D) 10.5B) 33.5 E) 286C) 62.5

____ 114) A slice of apple pie contains 14.0 grams of fat, 2.00 grams of protein, and 52.0 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If cycling typically burns 1000.0 kJ/hour, __________ minutes of cycling are required to completely burn off the slice of pie.

A) 1.45 D) 87.0B) 4.66 E) less than one minuteC) 8.25

____ 115) The kinetic energy of a 12.5-g object moving at a speed of 81.9 m/s is __________ J.A) 145 D) 41900B) 0.950 E) 1450C) 41.9

____ 116) The kinetic energy of a 23.2-g object moving at a speed of 93.6 m/s is __________ J.A) 145 D) 0.950B) 102 E) 102000C) 1450

____ 117) The value of E for a system that performs 168 kJ of work on its surroundings and loses 79 kJ of heat is __________ kJ.A) +247 D) -55B) -247 E) -168C) +55

____ 118) Calculate the value of E in joules for a system that loses 73 J of heat and has 150 J of work performed on it by the surroundings.A) -73 D) +223B) -77 E) -223C) +77

____ 119) The value of H° for the reaction below is -72 kJ. __________ kJ of heat are released when 4.0 mol of HBr is formed in this reaction.

H2 (g) + Br2 (g) 2HBr (g)A) 126 D) 144B) 72 E) -72C) 0.44

____ 120) The value of H° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 20.0 g of Na2O2 with water is __________ kJ.

2 Na2O2 (s) + 2 H2O (l) 4NaOH (s) + O2 (g)A) 16.2 D) 64.6B) 32.3 E) -126C) 67.5

____ 121) The value of ÄH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 6.00 g of CO (g) reacts completely.

2CO (g) + O2 (g) 2CO2 (g)A) 1450 D) 482B) 103 E) -482C) 51.6

____ 122) In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:

CH4 (g) + 2O2 (g) CO2 (g) + 2H2O (l) H = -890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.A) -94.6 D) 32.7B) 0.0306 E) -9.46 104

C) -0.0106

____ 123) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:

2H2O2 (l) 2H2O (l) + O2 (g) H = -196 kJ

Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?A) -23.1 D) 1.44B) -11.5 E) -2.31 104

C) -0.0217

____ 124) The combustion of titanium with oxygen produces titanium dioxide:

Ti (s) + O2 (g) TiO2 (s)

When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is __________ kJ/mol.A) 14.3 D) -0.154B) 19.6 E) -1.52 104

C) -311

____ 125) A sample of aluminum metal absorbs 8.32 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is __________ g.A) 72 D) 65B) 1.3 E) 7.3C) 7.5

____ 126) The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1 °C to 65.3 °C?A) 48.1 D) 2.08 10-2B) 840 E) 54.4C) 1.89 103

____ 127) The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0 °C to 75.0 °C?A) 88.6 D) 0.0113B) 429 E) 22.9C) 1221

____ 128) The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of mercury from 15.0 °C to 36.5 °C?A) 7.7 102 D) 0.0013B) 15 E) 1.7C) 36

____ 129) The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 °C to 77.5 °C?A) 1.79 105 D) 5.58 10-6

B) 26.6 E) 0.00558C) 2.66 104

____ 130) A 5.00-g sample of liquid water at 25.0 °C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.A) 95.2 D) 29.0B) 25.2 E) 4.02C) -21.0

____ 131) The ÄH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 10.1-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 °C to __________°C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.A) 35.2 D) 33.3

B) 24.0 E) 40.2C) 33.7

____ 132) A 50.0-g sample of liquid water at 25.0 °C is mixed with 29.0 g of water at 45.0 °C. The final temperature of the water is __________ °C.A) 102 D) 142B) 27.6 E) 32.3C) 35.0

____ 133) A 6.50-g sample of copper metal at 25.0 °C is heated by the addition of 84.0 J of energy. The final temperature of the copper is __________°C. The specific heat capacity of copper is 0.38 J/g-K.A) 29.9 D) 59.0B) 25.0 E) 34.0C) 9.0

____ 134) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.)A) -7.43 D) -9.12B) -12.51 E) 6.51C) 8.20

____ 135) A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 20.2 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is __________ kJ.A) 520 D) 720B) 630 E) 72C) 340

136) __________ is defined as the energy used to move an object against a force.

137) Given the equation

H2O (l) H2O (g) Hrxn = 40.7 kJ at 100 °C

Calculate the mass of liquid water (in grams) at 100 °C that can converted to vapor by absorbing 2400 J of heat.

138) Given the equation

H2O (l) H2O (g) Hrxn = 40.7 kJ at 100°C

Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.

139) When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is __________ J. (The specific heat of water is 4.18 J/g- °C.)

140) Given the equation:

CH4 (g) + 2 O2 (g) CO2 (g) + H2O (l) H = -890 kJ

The heat liberated when 34.78 grams of methane (CH4) are burned in an excess amount of oxygen is __________ kJ.

141) The standard enthalpy change of a reaction is the enthalpy change when all reactants and products are at ________ pressure and a specific temperature.

142) Coal contains hydrocarbons of high molecular weight as well as compounds containing ________, oxygen, or nitrogen.

____ 143) Work equals force times distance.

____ 144) One joule equals 1 kg · m2/s2.

____ 145) Units of energy include newtons, joules, and calories.

____ 146) The primary component of natural gas is propane.

____ 147) Renewable energy sources are essentially inexhaustible.

____ 148) Petroleum is a liquid composed of hundreds of compounds.

Chem II Practice TestAnswer Section

1) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.12) ANS: E PTS: 1 DIF: 1 REF: Sec. 5.13) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.24) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.25) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.26) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.27) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.28) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.29) ANS: E PTS: 1 DIF: 2 REF: Sec. 5.2

10) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.211) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.212) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.213) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.214) ANS: B PTS: 1 DIF: 1 REF: Sec. 5.315) ANS: C PTS: 1 DIF: 1 REF: Sec. 5.316) ANS: E PTS: 1 DIF: 1 REF: Sec. 5.317) ANS: C PTS: 1 DIF: 1 REF: Sec. 5.318) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.419) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.420) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.421) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.422) ANS: C PTS: 1 DIF: 1 REF: Sec. 5.423) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.424) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.525) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.526) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.527) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.528) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.529) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.530) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.531) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.532) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.533) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.634) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.735) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.736) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.737) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.738) ANS: A PTS: 1 DIF: 1 REF: Sec. 5.739) ANS: E PTS: 1 DIF: 1 REF: Sec. 5.7

40) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.741) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.742) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.743) ANS: E PTS: 1 DIF: 2 REF: Sec. 5.744) ANS: E PTS: 1 DIF: 2 REF: Sec. 5.745) ANS: E PTS: 1 DIF: 1 REF: Sec. 5.746) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.847) ANS: D PTS: 1 DIF: 1 REF: Sec. 5.848) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.849) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.850) ANS: C PTS: 1 DIF: 1 REF: Sec. 5.851) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.152) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.153) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.154) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.155) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.156) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.157) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.158) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.159) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.160) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.161) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.262) ANS: E PTS: 1 DIF: 2 REF: Sec. 5.263) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.264) ANS: A PTS: 1 DIF: 2 REF: Sec. 5.265) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.466) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.467) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.468) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.469) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.470) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.471) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.472) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.473) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.474) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.475) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.476) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.477) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.478) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.479) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.480) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.581) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.582) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.5

83) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.584) ANS: B PTS: 1 DIF: 4 REF: Sec. 5.585) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.686) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.687) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.688) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.689) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.690) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.691) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.692) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.693) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.694) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.695) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.796) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.797) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.798) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.799) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.7

100) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.7101) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.7102) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.7103) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.7104) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.7105) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.7106) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.7107) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.7108) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.7109) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.7110) ANS: C PTS: 1 DIF: 4 REF: Sec. 5.8111) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.8112) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.8113) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.8114) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.8115) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.1116) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.1117) ANS: B PTS: 1 DIF: 2 REF: Sec. 5.2118) ANS: C PTS: 1 DIF: 2 REF: Sec. 5.2119) ANS: D PTS: 1 DIF: 2 REF: Sec. 5.4120) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.4121) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.4122) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.4123) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.4124) ANS: E PTS: 1 DIF: 4 REF: Sec. 5.5125) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.5

126) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.5127) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.5128) ANS: B PTS: 1 DIF: 3 REF: Sec. 5.5129) ANS: C PTS: 1 DIF: 3 REF: Sec. 5.5130) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.5131) ANS: D PTS: 1 DIF: 4 REF: Sec. 5.5132) ANS: E PTS: 1 DIF: 3 REF: Sec. 5.5133) ANS: D PTS: 1 DIF: 3 REF: Sec. 5.5134) ANS: D PTS: 1 DIF: 4 REF: Sec. 5.5135) ANS: A PTS: 1 DIF: 3 REF: Sec. 5.8136) ANS:

Work

PTS: 1 DIF: 2 REF: Sec. 5.1137) ANS:

1.061 grams


6.78 kJ


868


1900


1 atm


sulfur

PTS: 1 DIF: 2 REF: Sec. 5.8143) ANS: T PTS: 1 DIF: 1 REF: Sec. 5.1144) ANS: T PTS: 1 DIF: 2 REF: Sec. 5.1145) ANS: F PTS: 1 DIF: 1 REF: Sec. 5.1146) ANS: F PTS: 1 DIF: 1 REF: Sec. 5.8147) ANS: T PTS: 1 DIF: 1 REF: Sec. 5.8148) ANS: T PTS: 1 DIF: 2 REF: Sec. 5.8

chem ii practice test chapter 5.docx

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