Question 1

Which of the following is the second law of thermodynamics?

Accepted Answer

A)  In a spontaneous process, the entropy of the universe increases. 
B)  There is no disorder in a perfect crystal at 0 K. 
C)  The total energy of the universe is always increasing. 
D)  The total energy of the universe is constant. 
E)  Mass and energy are conserved in all chemical reactions. 
A)  In a spontaneous process, the entropy of the universe increases. 
B)  There is no disorder in a perfect crystal at 0 K. 
C)  The total energy of the universe is always increasing. 
D)  The total energy of the universe is constant. 
E)  Mass and energy are conserved in all chemical reactions.

Question 2

In any chemical process, energy must be conserved. This is the _____ law of thermodynamics.

Accepted Answer

The answer of In any chemical process, energy must be...

Question 3

The change in entropy for any process is not dependent upon the pathway by which the process occurs. In other words, the change in entropy for any process is a(n) _____ function.

Accepted Answer

The answer of The change in entropy for any process...

Question 4

Which of the following represents the change in entropy for a system going from 142 possible microstates to 830 possible microstates? (k = 1.381 × 10-23 J/K)

Accepted Answer

A)  $1.61 \times 10 ^ { - 22 }$ J/K 
B)  $9.02 \times 10 ^ { - 23 }$ J/K 
C)  ? $9.02 \times 10 ^ { - 23 }$ J/K 
D)  $2.44 \times 10 ^ { - 23 }$ J/K 
E)  ? $2.44 \times 10 ^ { - 23 }$ J/K 
A)  $1.61 \times 10 ^ { - 22 }$ J/K 
B)  $9.02 \times 10 ^ { - 23 }$ J/K 
C)  ? $9.02 \times 10 ^ { - 23 }$ J/K 
D)  $2.44 \times 10 ^ { - 23 }$ J/K 
E)  ? $2.44 \times 10 ^ { - 23 }$ J/K

Question 5

While diluting concentrated sulfuric acid with water, the temperature of the solution increases rapidly. What are the signs of ΔrH, ΔrS, and ΔrG for the process?

Accepted Answer

A)  ΔrH rS > 0, and ΔrG rH rS rG rH rS > 0, and ΔrG > 0 
D)  ΔrH > 0, ΔrS > 0, and ΔrG rH > 0, ΔrS rG > 0 
A)  ΔrH rS > 0, and ΔrG rH rS rG rH rS > 0, and ΔrG > 0 
D)  ΔrH > 0, ΔrS > 0, and ΔrG rH > 0, ΔrS rG > 0

Question 6

Which of the following is the equilibrium constant for the reaction below at 25 °C? (R = 8.314 J/K ⋅mol) MgCO3(s) MgO(s) + CO2(g); ΔfG° [MgCO3(s)] = -1028.2 kJ/mol, ΔfG [MgO(s)] = -568.8 kJ/mol, and ΔfG° [CO2(g)] = -394.4 kJ/mol.

Accepted Answer

A)  4.0 × 10-12 
B)  0.97 
C)  1.0 
D)  1.0 × 104 
E)  2.5 × 1011 
A)  4.0 × 10-12 
B)  0.97 
C)  1.0 
D)  1.0 × 104 
E)  2.5 × 1011

Question 7

What is the equilibrium constant for the reaction below at 298 K? 
2C(s) + 3H2(g) ? C2H6(g)
Given: ?rH° = -84.68 kJ; ?rS° = -173.8 J/K at 298 K. (R = 8.314 J/K?mol)

Accepted Answer

A)  5.8 × 105 
B)  1.0 × 10?5 
C)  8.6 × 10-10 
D)  1.7 × 10-6 
E)  7.0 × 1014 
A)  5.8 × 105 
B)  1.0 × 10?5 
C)  8.6 × 10-10 
D)  1.7 × 10-6 
E)  7.0 × 1014

Question 8

Which of the following statements concerning entropy is not correct?

Accepted Answer

A)  The entropy of a system increases as the number of available microstates increases. 
B)  The entropy of a system is proportional to the natural log of the number of microstates. 
C)  In a spontaneous process, ΔS(universe) indicates the extent to which energy is dispersed. 
D)  The dispersal of matter, such as the spontaneous expansion of a gas, cannot be explained by an increase in entropy. 
E)  Entropy is a measure of the extent of energy dispersal. 
A)  The entropy of a system increases as the number of available microstates increases. 
B)  The entropy of a system is proportional to the natural log of the number of microstates. 
C)  In a spontaneous process, ΔS(universe) indicates the extent to which energy is dispersed. 
D)  The dispersal of matter, such as the spontaneous expansion of a gas, cannot be explained by an increase in entropy. 
E)  Entropy is a measure of the extent of energy dispersal.

Question 9

The standard entropy for the formation of sulfur hexafluoride from the sulfur and fluorine is -348.7 J/K ⋅mol-rxn at 298.15 K. What is the standard molar entropy of sulfur hexafluoride for the reaction below? (Given: S°[S(s)] = 32.1 J/K ⋅mol and S°[F2(g)] = 202.8 J/K ⋅mol)

Accepted Answer

A)  -988.6 J/K⋅mol 
B)  +291.8 J/K⋅mol 
C)  -291.8 J/K⋅mol 
D)  -113.2 J/K⋅mol 
E)  +113.8 J/K⋅mol 
A)  -988.6 J/K⋅mol 
B)  +291.8 J/K⋅mol 
C)  -291.8 J/K⋅mol 
D)  -113.2 J/K⋅mol 
E)  +113.8 J/K⋅mol

Question 10

The dissolution of ammonium nitrate occurs spontaneously in water at 25 °C. As ammonium nitrate dissolves, the temperature of the water decreases. What are the signs of ΔrH, ΔrS, and ΔrG for this process?

Accepted Answer

A)  ΔrH > 0, ΔrS rG > 0 
B)  ΔrH > 0, ΔrS > 0, and ΔrG > 0 
C)  ΔrH > 0, ΔrS > 0, and ΔrG rH rS rG rH rS > 0, and ΔrG > 0 
A)  ΔrH > 0, ΔrS rG > 0 
B)  ΔrH > 0, ΔrS > 0, and ΔrG > 0 
C)  ΔrH > 0, ΔrS > 0, and ΔrG rH rS rG rH rS > 0, and ΔrG > 0

Which of the following is the second law of thermodynamics?

In any chemical process, energy must be conserved. This is the _____ law of thermodynamics.

The change in entropy for any process is not dependent upon the pathway by which the process occurs. In other words, the change in entropy for any process is a(n) _____ function.

Which of the following represents the change in entropy for a system going from 142 possible microstates to 830 possible microstates? (k = 1.381 × 10^-23 J/K)

While diluting concentrated sulfuric acid with water, the temperature of the solution increases rapidly. What are the signs of ΔrH, ΔrS, and ΔrG for the process?

Which of the following is the equilibrium constant for the reaction below at 25 °C? (R = 8.314 J/K ⋅mol) MgCO3(s) MgO(s) + CO2(g); ΔfG° [MgCO3(s)] = -1028.2 kJ/mol, ΔfG [MgO(s)] = -568.8 kJ/mol, and ΔfG° [CO2(g)] = -394.4 kJ/mol.

What is the equilibrium constant for the reaction below at 298 K? 2C(s) + 3H₂(g) ? C₂H₆(g) Given: ?_rH° = -84.68 kJ; ?_rS° = -173.8 J/K at 298 K. (R = 8.314 J/K?mol)

Which of the following statements concerning entropy is not correct?

The standard entropy for the formation of sulfur hexafluoride from the sulfur and fluorine is -348.7 J/K ⋅mol-rxn at 298.15 K. What is the standard molar entropy of sulfur hexafluoride for the reaction below? (Given: S°[S(s)] = 32.1 J/K ⋅mol and S°[F2(g)] = 202.8 J/K ⋅mol)

The dissolution of ammonium nitrate occurs spontaneously in water at 25 °C. As ammonium nitrate dissolves, the temperature of the water decreases. What are the signs of Δ_rH, Δ_rS, and Δ_rG for this process?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Exam 19: Principles of Chemical Reactivity: Entropy and Free Energy

Which of the following is the second law of thermodynamics?

In any chemical process, energy must be conserved. This is the _____ law of thermodynamics.

The change in entropy for any process is not dependent upon the pathway by which the process occurs. In other words, the change in entropy for any process is a(n) _____ function.

Which of the following represents the change in entropy for a system going from 142 possible microstates to 830 possible microstates? (k = 1.381 × 10-23 J/K)

While diluting concentrated sulfuric acid with water, the temperature of the solution increases rapidly. What are the signs of ΔrH, ΔrS, and ΔrG for the process?

Which of the following is the equilibrium constant for the reaction below at 25 °C? (R = 8.314 J/K ⋅mol) MgCO3(s) MgO(s) + CO2(g); ΔfG° [MgCO3(s)] = -1028.2 kJ/mol, ΔfG [MgO(s)] = -568.8 kJ/mol, and ΔfG° [CO2(g)] = -394.4 kJ/mol.

What is the equilibrium constant for the reaction below at 298 K? 2C(s) + 3H2(g) ? C2H6(g) Given: ?rH° = -84.68 kJ; ?rS° = -173.8 J/K at 298 K. (R = 8.314 J/K?mol)

Which of the following statements concerning entropy is not correct?

The standard entropy for the formation of sulfur hexafluoride from the sulfur and fluorine is -348.7 J/K ⋅mol-rxn at 298.15 K. What is the standard molar entropy of sulfur hexafluoride for the reaction below? (Given: S°[S(s)] = 32.1 J/K ⋅mol and S°[F2(g)] = 202.8 J/K ⋅mol)

The dissolution of ammonium nitrate occurs spontaneously in water at 25 °C. As ammonium nitrate dissolves, the temperature of the water decreases. What are the signs of ΔrH, ΔrS, and ΔrG for this process?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Which of the following represents the change in entropy for a system going from 142 possible microstates to 830 possible microstates? (k = 1.381 × 10^-23 J/K)

What is the equilibrium constant for the reaction below at 298 K? 2C(s) + 3H₂(g) ? C₂H₆(g) Given: ?_rH° = -84.68 kJ; ?_rS° = -173.8 J/K at 298 K. (R = 8.314 J/K?mol)

The dissolution of ammonium nitrate occurs spontaneously in water at 25 °C. As ammonium nitrate dissolves, the temperature of the water decreases. What are the signs of Δ_rH, Δ_rS, and Δ_rG for this process?