Question 1

The internal energy of a system __________.

Accepted Answer

A) is the sum of the kinetic energy of all of its components 
B) is the sum of the rotational, vibrational, and translational energies of all of its components 
C) refers only to the energies of the nuclei of the atoms of the component molecules 
D) is the sum of the potential and kinetic energies of the components 
E) none of the above 
A) is the sum of the kinetic energy of all of its components 
B) is the sum of the rotational, vibrational, and translational energies of all of its components 
C) refers only to the energies of the nuclei of the atoms of the component molecules 
D) is the sum of the potential and kinetic energies of the components 
E) none of the above

Question 2

For which one of the following reactions is the value of ΔH°rxn equal to ΔH°f for the product?

Accepted Answer

A) H2O (l)+ 1/2 O2 (g)→ H2 O2 (l) 
B) N2 (g)+ O2 (g)→ 2NO (g) 
C) 2H2 (g)+ O2 (g)→ 2H2O (l) 
D) 2H2 (g)+ O2 (g)→ 2H2O (g) 
E) none of the above 
A) H2O (l)+ 1/2 O2 (g)→ H2 O2 (l) 
B) N2 (g)+ O2 (g)→ 2NO (g) 
C) 2H2 (g)+ O2 (g)→ 2H2O (l) 
D) 2H2 (g)+ O2 (g)→ 2H2O (g) 
E) none of the above

Question 3

The value of ΔH° 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)

Accepted Answer

A) 16.2 
B) 32.3 
C) 67.5 
D) 64.6 
E) -126 
A) 16.2 
B) 32.3 
C) 67.5 
D) 64.6 
E) -126

Question 4

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.

Accepted Answer

A) 4.78 
B) 33.5 
C) 62.5 
D) 10.5 
E) 286 
A) 4.78 
B) 33.5 
C) 62.5 
D) 10.5 
E) 286

Question 5

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

Accepted Answer

A) a only 
B) b only 
C) c only 
D) a and c 
E) a and b 
A) a only 
B) b only 
C) c only 
D) a and c 
E) a and b

Question 6

The value of ΔE for a system that performs 168 kJ of work on its surroundings and loses 79 kJ of heat is __________ kJ.

Accepted Answer

A) +247 
B) -247 
C) +55 
D) -55 
E) -168 
A) +247 
B) -247 
C) +55 
D) -55 
E) -168

Question 7

The units of of heat capacity are __________.

Accepted Answer

A) K/J or °C/J 
B) J/K or J/°C 
C) J/g-K or J/g-°C 
D) J/mol 
E) g-K/J or g-°C/J 
A) K/J or °C/J 
B) J/K or J/°C 
C) J/g-K or J/g-°C 
D) J/mol 
E) g-K/J or g-°C/J

Question 8

Given the equation:
CH4 (g)+ 2 O2 (g)→ CO2 (g)+ H2O (l)ΔH = -890 kJ
The heat liberated when 34.78 grams of methane (CH4)are burned in an excess amount of oxygen is __________ kJ.

Accepted Answer

Question 9

Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

Accepted Answer

A) 3.60 × 106 
B) 1.20 × 104 
C) 3.60 × 103 
D) 12.0 
E) 80.0 
A) 3.60 × 106 
B) 1.20 × 104 
C) 3.60 × 103 
D) 12.0 
E) 80.0

Question 10

The kinetic energy of a 23.2-g object moving at a speed of 93.6 m/s is __________ J.

Accepted Answer

A) 145 
B) 102 
C) 1450 
D) 0.950 
E) 102000 
A) 145 
B) 102 
C) 1450 
D) 0.950 
E) 102000

Question 11

Calculate the value of ΔE in joules for a system that loses 73 J of heat and has 150 J of work performed on it by the surroundings.

Accepted Answer

A) -73 
B) -77 
C) +77 
D) +223 
E) -223 
A) -73 
B) -77 
C) +77 
D) +223 
E) -223

Question 12

Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph.

Accepted Answer

A) 1.2 × 104 
B) 2.9 × 105 
C) 5.9 × 105 
D) 3.2 × 106 
E) 3.2 × 10-6 
A) 1.2 × 104 
B) 2.9 × 105 
C) 5.9 × 105 
D) 3.2 × 106 
E) 3.2 × 10-6

Question 13

Given the following reactions CaCO3 (s)→ CaO (s)+ CO2 (g)ΔH = 178.1 kJ
C (s, graphite)+ O2 (g)→ CO2 (g)ΔH = -393.5 kJ
The enthalpy of the reaction
CaCO3 (s)→ CaO (s)+ C (s, graphite)+ O2 (g)
Is __________ kJ.

Accepted Answer

A) 215.4 
B) 571.6 
C) -215.4 
D) -571.6 
E) 7.01 × 104 
A) 215.4 
B) 571.6 
C) -215.4 
D) -571.6 
E) 7.01 × 104

Question 14

For which one of the following equations is ΔH°rxn equal to ΔHf° for the product?

Accepted Answer

A) Xe (g)+ 2 F2 (g)→ XeF4 (g) 
B) CH4 (g)+ 2 Cl2 (g)→ CH2 Cl2 (l)+ 2HCl (g) 
C) N2 (g)+ O3 (g)→ N2O3 (g) 
D) 2CO (g)+ O2 (g)→ 2CO2 (g) 
E) C (diamond)+ O2 (g)→ CO2 (g) 
A) Xe (g)+ 2 F2 (g)→ XeF4 (g) 
B) CH4 (g)+ 2 Cl2 (g)→ CH2 Cl2 (l)+ 2HCl (g) 
C) N2 (g)+ O3 (g)→ N2O3 (g) 
D) 2CO (g)+ O2 (g)→ 2CO2 (g) 
E) C (diamond)+ O2 (g)→ CO2 (g)

Question 15

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.

Accepted Answer

A) 10,155 
B) 5,155 
C) -5,155 
D) -10,155 
E) 1.91 ×   
A) 10,155 
B) 5,155 
C) -5,155 
D) -10,155 
E) 1.91 ×

Question 16

Which one of the following is an endothermic process?

Accepted Answer

A) ice melting 
B) water freezing 
C) boiling soup 
D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases. 
E) Both A and C 
A) ice melting 
B) water freezing 
C) boiling soup 
D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases. 
E) Both A and C

Question 17

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.

Accepted Answer

A) 95.2 
B) 25.2 
C) -21.0 
D) 29.0 
E) 4.02 
A) 95.2 
B) 25.2 
C) -21.0 
D) 29.0 
E) 4.02

Question 18

Given the data in the table below, ΔH° for the reaction 2CO (g)+ O2 (g)→ 2CO2 (g)
Is __________ kJ.

Accepted Answer

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

Question 19

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

Accepted Answer

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

Question 20

Objects can possess energy as __________. (a)endothermic energy
(b)potential energy
(c)kinetic energy

Accepted Answer

A) a only 
B) b only 
C) c only 
D) a and c 
E) b and c 
A) a only 
B) b only 
C) c only 
D) a and c 
E) b and c

Exam 5: Thermochemistry

The internal energy of a system __________.

For which one of the following reactions is the value of ΔH°rxn equal to ΔH°f for the product?

The value of ΔH° 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)

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

The value of ΔE for a system that performs 168 kJ of work on its surroundings and loses 79 kJ of heat is __________ kJ.

The units of of heat capacity are __________.

Given the equation: CH4 (g)+ 2 O2 (g)→ CO2 (g)+ H2O (l)ΔH = -890 kJ The heat liberated when 34.78 grams of methane (CH4)are burned in an excess amount of oxygen is __________ kJ.

Calculate the kinetic energy in joules of an 80.0 g bullet traveling at 300.0 m/s.

The kinetic energy of a 23.2-g object moving at a speed of 93.6 m/s is __________ J.

Calculate the value of ΔE in joules for a system that loses 73 J of heat and has 150 J of work performed on it by the surroundings.

Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph.

Given the following reactions CaCO3 (s)→ CaO (s)+ CO2 (g)ΔH = 178.1 kJ C (s, graphite)+ O2 (g)→ CO2 (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO3 (s)→ CaO (s)+ C (s, graphite)+ O2 (g) Is __________ kJ.

For which one of the following equations is ΔH°rxn equal to ΔHf° for the product?

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.

Which one of the following is an endothermic process?

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.

Given the data in the table below, ΔH° for the reaction 2CO (g)+ O2 (g)→ 2CO2 (g) Is __________ kJ.

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

Objects can possess energy as __________. (a)endothermic energy (b)potential energy (c)kinetic energy

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

For which one of the following reactions is the value of ΔH°_rxn equal to ΔH°_f for the product?

The value of ΔH° 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)

Given the equation: CH₄ (g)+ 2 O₂ (g)→ CO₂ (g)+ H₂O (l)ΔH = -890 kJ The heat liberated when 34.78 grams of methane (CH₄)are burned in an excess amount of oxygen is __________ kJ.

Given the following reactions CaCO₃ (s)→ CaO (s)+ CO₂ (g)ΔH = 178.1 kJ C (s, graphite)+ O₂ (g)→ CO₂ (g)ΔH = -393.5 kJ The enthalpy of the reaction CaCO₃ (s)→ CaO (s)+ C (s, graphite)+ O₂ (g) Is __________ kJ.

For which one of the following equations is ΔH°_rxn equal to ΔH_f° for the product?

Given the data in the table below, ΔH° for the reaction 2CO (g)+ O₂ (g)→ 2CO₂ (g) Is __________ kJ.

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