Question 1

Why is the quantity of energy required to recharge a battery greater than the quantity of work done?

Accepted Answer

Some of th

Question 2

Identify the change in state that does not have an increase in entropy.

Accepted Answer

A)  water freezing 
B)  water boiling 
C)  ice melting 
D)  dry ice subliming 
E)  water evaporating 
A)  water freezing 
B)  water boiling 
C)  ice melting 
D)  dry ice subliming 
E)  water evaporating

Question 3

In which of the following processes do the molecules become more ordered?

Accepted Answer

A)  water freezing 
B)  ice melting 
C)  water evaporating 
D)  salt dissolving in water 
E)  dry ice subliming 
A)  water freezing 
B)  ice melting 
C)  water evaporating 
D)  salt dissolving in water 
E)  dry ice subliming

Question 4

Determine the equilibrium constant for the following reaction at 498 K: 2 Hg(g) + O2(g) → 2HgO(s) ΔrH° = -304.2 kJ mol-1; ΔrS° = -414.2 J K-1 mol-1

Accepted Answer

A)  1.87 × 1010 
B)  8.10 × 1031 
C)  2.31 × 10-22 
D)  5.34 × 10-11 
E)  4.33 × 1021 
A)  1.87 × 1010 
B)  8.10 × 1031 
C)  2.31 × 10-22 
D)  5.34 × 10-11 
E)  4.33 × 1021

Question 5

For the following example, what is true about ΔrH and ΔrS? 2N2O(g) → 2N2(g) + O2(g)

Accepted Answer

A)  a negative ΔrH and a negative ΔrS 
B)  a positive ΔrH and a negative ΔrS 
C)  a negative ΔrH and a positive ΔrS 
D)  a positive ΔrH and a positive ΔrS 
E)  ΔrH = 0 and a positive ΔrS 
A)  a negative ΔrH and a negative ΔrS 
B)  a positive ΔrH and a negative ΔrS 
C)  a negative ΔrH and a positive ΔrS 
D)  a positive ΔrH and a positive ΔrS 
E)  ΔrH = 0 and a positive ΔrS

Question 6

Consider a reaction that has a positive ΔrH and a positive ΔrS. Which of the following statements is TRUE?

Accepted Answer

A)  This reaction will be spontaneous only at high temperatures. 
B)  This reaction will be spontaneous at all temperatures. 
C)  This reaction will be nonspontaneous at all temperatures. 
D)  This reaction will be nonspontaneous only at high temperatures. 
E)  This reaction will be spontaneous only at very low temperatures. 
A)  This reaction will be spontaneous only at high temperatures. 
B)  This reaction will be spontaneous at all temperatures. 
C)  This reaction will be nonspontaneous at all temperatures. 
D)  This reaction will be nonspontaneous only at high temperatures. 
E)  This reaction will be spontaneous only at very low temperatures.

Question 7

What is the name of the reaction that does not achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Accepted Answer

A)  reversible reaction 
B)  forward reaction 
C)  reverse reaction 
D)  equilibrium reaction 
E)  irreversible reaction 
A)  reversible reaction 
B)  forward reaction 
C)  reverse reaction 
D)  equilibrium reaction 
E)  irreversible reaction

Question 8

Determine ΔrG° at 298 K using the following information: H2(g) + CO(g) → CH2O(g) ΔrH°= +1.9 kJ mol-1; ΔrS°= -109.6 J K-1 mol-1

Accepted Answer

A)  +57.7 kJ mol-1 
B)  -30.8 kJ mol-1 
C)  +34.6 kJ mol-1 
D)  -41.5 kJ mol-1 
E)  +17.3 kJ mol-1 
A)  +57.7 kJ mol-1 
B)  -30.8 kJ mol-1 
C)  +34.6 kJ mol-1 
D)  -41.5 kJ mol-1 
E)  +17.3 kJ mol-1

Question 9

Define entropy.

Accepted Answer

Entropy is a thermodynamic fun

Question 10

Phosphorus and chlorine gases combine to produce phosphorus trichloride:   (g) +   (g) →   (g) ΔrG° at 298 K for this reaction is -642.9 kJ mol-1. The value of ΔrG at 298 K for a reaction mixture that consists of     and   is ________ kJ mol-1.

Accepted Answer

A)  -5.51 × 103 
B)  -90.0 
C)  -71.1 
D)  -4.87 × 103 
E)  -647.8 
A)  -5.51 × 103 
B)  -90.0 
C)  -71.1 
D)  -4.87 × 103 
E)  -647.8

Question 11

Estimate ΔrG° for the following reaction at 387 K. HCN(g) + 2H2(g) → CH3NH2(g) ΔrH°= -158.0 kJ mol-1; ΔrS°= -219.9 J K-1 mol-1

Accepted Answer

A)  +243 kJ mol-1 
B)  -72.9 kJ mol-1 
C)  +84.9 kJ mol-1 
D)  -92.5 kJ mol-1 
E)  -188 kJ mol-1 
A)  +243 kJ mol-1 
B)  -72.9 kJ mol-1 
C)  +84.9 kJ mol-1 
D)  -92.5 kJ mol-1 
E)  -188 kJ mol-1

Question 12

Match the following.
-Q = 1

Accepted Answer

A) standard state 
B) equilibrium 
C) ΔrG > ΔrG° 
D) ΔrG > 0 
E) DrG rG rG° 
A) standard state 
B) equilibrium 
C) ΔrG > ΔrG° 
D) ΔrG > 0 
E) DrG rG rG°

Question 13

Calculate the equilibrium constant for the following reaction at 298 K: 2H2S(g) → 2H2(g) + S2(g) ΔrH° = 169.8 kJ mol-1; ΔrS°= 78.0 J K-1 mol-1

Accepted Answer

A)  3.28 × 10-21 
B)  4.99 × 10-29 
C)  1.05 × 10-25 
D)  2.06 × 10-26 
E)  6.38 × 10-24 
A)  3.28 × 10-21 
B)  4.99 × 10-29 
C)  1.05 × 10-25 
D)  2.06 × 10-26 
E)  6.38 × 10-24

Question 14

Determine the temperature of a reaction if ΔrG = -24.3 kJ mol-1, ΔrG° = -68.1 kJ mol-1, and Q = 218

Accepted Answer

A)  304 K 
B)  298 K 
C)  621 K 
D)  978 K 
E)  345 K 
A)  304 K 
B)  298 K 
C)  621 K 
D)  978 K 
E)  345 K

Why is the quantity of energy required to recharge a battery greater than the quantity of work done?

Identify the change in state that does not have an increase in entropy.

In which of the following processes do the molecules become more ordered?

Determine the equilibrium constant for the following reaction at 498 K: 2 Hg(g) + O₂(g) → 2HgO(s) Δ_rH° = -304.2 kJ mol^-1; Δ_rS° = -414.2 J K^-1 mol^-1

For the following example, what is true about Δ_rH and Δ_rS? 2N₂O(g) → 2N₂(g) + O₂(g)

Consider a reaction that has a positive Δ_rH and a positive Δ_rS. Which of the following statements is TRUE?

What is the name of the reaction that does not achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Define entropy.

Phosphorus and chlorine gases combine to produce phosphorus trichloride: (g) + (g) → (g) Δ_rG° at 298 K for this reaction is -642.9 kJ mol^-1. The value of Δ_rG at 298 K for a reaction mixture that consists of and is ________ kJ mol^-1.

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

Match the following. -Q = 1

Calculate the equilibrium constant for the following reaction at 298 K: 2H₂S(g) → 2H₂(g) + S₂(g) Δ_rH° = 169.8 kJ mol^-1; Δ_rS°= 78.0 J K^-1 mol^-1

Determine the temperature of a reaction if Δ_rG = -24.3 kJ mol^-1, Δ_rG° = -68.1 kJ mol^-1, and Q = 218

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Exam 17: Gibbs Energy and Thermodynamics

Why is the quantity of energy required to recharge a battery greater than the quantity of work done?

Identify the change in state that does not have an increase in entropy.

In which of the following processes do the molecules become more ordered?

Determine the equilibrium constant for the following reaction at 498 K: 2 Hg(g) + O2(g) → 2HgO(s) ΔrH° = -304.2 kJ mol-1; ΔrS° = -414.2 J K-1 mol-1

For the following example, what is true about ΔrH and ΔrS? 2N2O(g) → 2N2(g) + O2(g)

Consider a reaction that has a positive ΔrH and a positive ΔrS. Which of the following statements is TRUE?

What is the name of the reaction that does not achieve the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Determine ΔrG° at 298 K using the following information: H2(g) + CO(g) → CH2O(g) ΔrH°= +1.9 kJ mol-1; ΔrS°= -109.6 J K-1 mol-1

Define entropy.

Phosphorus and chlorine gases combine to produce phosphorus trichloride: (g) + (g) → (g) ΔrG° at 298 K for this reaction is -642.9 kJ mol-1. The value of ΔrG at 298 K for a reaction mixture that consists of and is ________ kJ mol-1.

Estimate ΔrG° for the following reaction at 387 K. HCN(g) + 2H2(g) → CH3NH2(g) ΔrH°= -158.0 kJ mol-1; ΔrS°= -219.9 J K-1 mol-1

Match the following. -Q = 1

Calculate the equilibrium constant for the following reaction at 298 K: 2H2S(g) → 2H2(g) + S2(g) ΔrH° = 169.8 kJ mol-1; ΔrS°= 78.0 J K-1 mol-1

Determine the temperature of a reaction if ΔrG = -24.3 kJ mol-1, ΔrG° = -68.1 kJ mol-1, and Q = 218

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Determine the equilibrium constant for the following reaction at 498 K: 2 Hg(g) + O₂(g) → 2HgO(s) Δ_rH° = -304.2 kJ mol^-1; Δ_rS° = -414.2 J K^-1 mol^-1

For the following example, what is true about Δ_rH and Δ_rS? 2N₂O(g) → 2N₂(g) + O₂(g)

Consider a reaction that has a positive Δ_rH and a positive Δ_rS. Which of the following statements is TRUE?

Determine Δ_rG° at 298 K using the following information: H₂(g) + CO(g) → CH₂O(g) Δ_rH°= +1.9 kJ mol^-1; Δ_rS°= -109.6 J K^-1mol^-1

Phosphorus and chlorine gases combine to produce phosphorus trichloride: (g) + (g) → (g) Δ_rG° at 298 K for this reaction is -642.9 kJ mol^-1. The value of Δ_rG at 298 K for a reaction mixture that consists of and is ________ kJ mol^-1.

Estimate Δ_rG° for the following reaction at 387 K. HCN(g) + 2H₂(g) → CH₃NH₂(g) Δ_rH°= -158.0 kJ mol^-1; Δ_rS°= -219.9 J K^-1 mol^-1

Calculate the equilibrium constant for the following reaction at 298 K: 2H₂S(g) → 2H₂(g) + S₂(g) Δ_rH° = 169.8 kJ mol^-1; Δ_rS°= 78.0 J K^-1 mol^-1

Determine the temperature of a reaction if Δ_rG = -24.3 kJ mol^-1, Δ_rG° = -68.1 kJ mol^-1, and Q = 218