Question 1

Of the following, which one is a state function?

Accepted Answer

A) H 
B) q 
C) w 
D) heat 
E) none of the above 
A) H 
B) q 
C) w 
D) heat 
E) none of the above

Question 2

Units of energy include newtons, joules, and calories.

Accepted Answer

A) True 
 B)False

Question 3

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)

Accepted Answer

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

Question 4

Of the following, ΔHf° is not zero for __________.

Accepted Answer

A) O2 (g) 
B) C (graphite) 
C) N2 (g) 
D) F2 (s) 
E) Cl2 (g) 
A) O2 (g) 
B) C (graphite) 
C) N2 (g) 
D) F2 (s) 
E) Cl2 (g)

Question 5

ΔH for the reaction IF5 (g)→ IF3 (g)+ F2 (g)
Is __________ kJ, give the data below.
IF (g)+ F2 (g)→ IF3 (g)ΔH = -390 kJ
IF (g)+ 2 F2 (g)→ IF5 (g)ΔH = -745 kJ

Accepted Answer

A) +355 
B) -1135 
C) +1135 
D) +35 
E) -35 
A) +355 
B) -1135 
C) +1135 
D) +35 
E) -35

Question 6

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.

Accepted Answer

A) 3415 
B) 60.29 
C) 1054 
D) 5.120 × 10-3 
E) Additional information is needed to complete the calculation. 
A) 3415 
B) 60.29 
C) 1054 
D) 5.120 × 10-3 
E) Additional information is needed to complete the calculation.

Question 7

Given the data in the table below, ΔH°rxn for the reaction 3 Cl2 (g)+ PH3 (g)→ PCl3 (g)+ 3 HCl (g)
Is __________ kJ.

Accepted Answer

A) -385.77 
B) -570.37 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation. 
A) -385.77 
B) -570.37 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation.

Question 8

Petroleum is a liquid composed of hundreds of compounds.

Accepted Answer

A) True 
 B)False

Question 9

When a system __________, ΔE is always negative.

Accepted Answer

A) absorbs heat and does work 
B) gives off heat and does work 
C) absorbs heat and has work done on it 
D) gives off heat and has work done on it 
E) none of the above is always negative. 
A) absorbs heat and does work 
B) gives off heat and does work 
C) absorbs heat and has work done on it 
D) gives off heat and has work done on it 
E) none of the above is always negative.

Question 10

The reaction 4Al (s)+ 3O2 (g)→ 2 Al2O3 (s)ΔH° = -3351 kJ
Is __________, and therefore heat is __________ by the reaction.

Accepted Answer

A) endothermic, released 
B) endothermic, absorbed 
C) exothermic, released 
D) exothermic, absorbed 
E) thermoneutral, neither released nor absorbed 
A) endothermic, released 
B) endothermic, absorbed 
C) exothermic, released 
D) exothermic, absorbed 
E) thermoneutral, neither released nor absorbed

Question 11

The value of ΔH° for the reaction below is +128.1 kJ: 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?

Accepted Answer

A) 162 
B) 62.0 
C) 128 
D) 653 
E) 326 
A) 162 
B) 62.0 
C) 128 
D) 653 
E) 326

Question 12

The value of ΔH° for the reaction below is +128.1 kJ: 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?

Accepted Answer

A) 0.182 
B) 162 
C) 8.31 
D) 23.3 
E) 62.0 
A) 0.182 
B) 162 
C) 8.31 
D) 23.3 
E) 62.0

Question 13

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.

Accepted Answer

A) 29.9 
B) 25.0 
C) 9.0 
D) 59.0 
E) 34.0 
A) 29.9 
B) 25.0 
C) 9.0 
D) 59.0 
E) 34.0

Question 14

Of the substances below, the highest fuel value is obtained from __________.

Accepted Answer

A) charcoal 
B) bituminous coal 
C) natural gas 
D) hydrogen 
E) wood 
A) charcoal 
B) bituminous coal 
C) natural gas 
D) hydrogen 
E) wood

Question 15

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?

Accepted Answer

A) 4.3 
B) 92 
C) 0.450 
D) 1100 
E) 1.1 x 103 
A) 4.3 
B) 92 
C) 0.450 
D) 1100 
E) 1.1 x 103

Question 16

Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2 H3AsO4 → Ca(H2AsO4)2 + 2 H2O
Is __________ kJ.

Accepted Answer

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

Question 17

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.

Accepted Answer

A) 72 
B) 1.3 
C) 7.5 
D) 65 
E) 7.3 
A) 72 
B) 1.3 
C) 7.5 
D) 65 
E) 7.3

Question 18

Given the data in the table below and ΔH°rxn for the reaction SO2Cl2 (g)+ 2 H2O (l)→ H2SO4 (l)+ 2HCl (g)ΔH° = -62 kJ
ΔH°f of HCl (g)is __________ kJ/mol.

Accepted Answer

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

Question 19

The specific heat of bromine liquid is 0.226 J/g ∙ K. The molar heat capacity (in J/mol-K)of bromine liquid is __________.

Accepted Answer

A) 707 
B) 36.1 
C) 18.1 
D) 9.05 
E) 0.226 
A) 707 
B) 36.1 
C) 18.1 
D) 9.05 
E) 0.226

Question 20

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?

Accepted Answer

A) 7.7 × 102 
B) 15 
C) 36 
D) 0.0013 
E) 1.7 
A) 7.7 × 102 
B) 15 
C) 36 
D) 0.0013 
E) 1.7

Exam 5: Thermochemistry

Of the following, which one is a state function?

Units of energy include newtons, joules, and calories.

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)

Of the following, ΔHf° is not zero for __________.

ΔH for the reaction IF5 (g)→ IF3 (g)+ F2 (g) Is __________ kJ, give the data below. IF (g)+ F2 (g)→ IF3 (g)ΔH = -390 kJ IF (g)+ 2 F2 (g)→ IF5 (g)ΔH = -745 kJ

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.

Given the data in the table below, ΔH°rxn for the reaction 3 Cl2 (g)+ PH3 (g)→ PCl3 (g)+ 3 HCl (g) Is __________ kJ.

Petroleum is a liquid composed of hundreds of compounds.

When a system __________, ΔE is always negative.

The reaction 4Al (s)+ 3O2 (g)→ 2 Al2O3 (s)ΔH° = -3351 kJ Is __________, and therefore heat is __________ by the reaction.

The value of ΔH° for the reaction below is +128.1 kJ: 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?

The value of ΔH° for the reaction below is +128.1 kJ: 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 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.

Of the substances below, the highest fuel value is obtained from __________.

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?

Given the data in the table below, ΔH°rxn for the reaction Ca(OH)2 + 2 H3AsO4 → Ca(H2AsO4)2 + 2 H2O Is __________ kJ.

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.

Given the data in the table below and ΔH°rxn for the reaction SO2Cl2 (g)+ 2 H2O (l)→ H2SO4 (l)+ 2HCl (g)ΔH° = -62 kJ ΔH°f of HCl (g)is __________ kJ/mol.

The specific heat of bromine liquid is 0.226 J/g ∙ K. The molar heat capacity (in J/mol-K)of bromine liquid is __________.

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?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

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)

Of the following, ΔH_f° is not zero for __________.

ΔH for the reaction IF₅ (g)→ IF₃ (g)+ F₂ (g) Is __________ kJ, give the data below. IF (g)+ F₂ (g)→ IF₃ (g)ΔH = -390 kJ IF (g)+ 2 F₂ (g)→ IF₅ (g)ΔH = -745 kJ

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.

Given the data in the table below, ΔH°_rxn for the reaction 3 Cl₂ (g)+ PH₃ (g)→ PCl₃ (g)+ 3 HCl (g) Is __________ kJ.

The reaction 4Al (s)+ 3O₂ (g)→ 2 Al₂O₃ (s)ΔH° = -3351 kJ Is , and therefore heat is by the reaction.

The value of ΔH° for the reaction below is +128.1 kJ: 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?

The value of ΔH° for the reaction below is +128.1 kJ: 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?

Given the data in the table below, ΔH°_rxn for the reaction Ca(OH)₂ + 2 H₃AsO₄ → Ca(H₂AsO₄)₂ + 2 H₂O Is __________ kJ.

Given the data in the table below and ΔH°_rxn for the reaction SO₂Cl₂ (g)+ 2 H₂O (l)→ H₂SO₄ (l)+ 2HCl (g)ΔH° = -62 kJ ΔH°_f of HCl (g)is __________ kJ/mol.