Question 1

Which of the following statements is TRUE?

Accepted Answer

A) A spontaneous reaction is a reaction that takes place without any outside intervention. 
B) Thermodynamics is a study of reaction rates. 
C) A nonspontaneous reaction is a reaction that does not take place under any conditions. 
D) Chemical kinetics is a discipline that studies the spontaneity of chemical reactions. 
E) Every spontaneous reaction is a very rapid reaction. 
A) A spontaneous reaction is a reaction that takes place without any outside intervention. 
B) Thermodynamics is a study of reaction rates. 
C) A nonspontaneous reaction is a reaction that does not take place under any conditions. 
D) Chemical kinetics is a discipline that studies the spontaneity of chemical reactions. 
E) Every spontaneous reaction is a very rapid reaction.

Question 2

Use the following thermodynamic values to calculate ?r  $G ^ { 0 }$ .
$\Delta_{r}$$ H^{\circ} $ = -95 kJ $\mathrm { mol } ^ { - 1 }$ ,$\Delta_{r}$$S ^ { 0 }$ = -157 J $\mathrm { mol } ^ { - 1 }$ ,T = 855 K

Accepted Answer

A) -48 kJ $\mathrm { mol } ^ { - 1 }$ 
B) -68 kJ $\mathrm { mol } ^ { - 1 }$ 
C) +39 kJ $\mathrm { mol } ^ { - 1 }$ 
D) -157 kJ $\mathrm { mol } ^ { - 1 }$ 
E) +142 kJ $\mathrm { mol } ^ { - 1 }$ 
A) -48 kJ $\mathrm { mol } ^ { - 1 }$ 
B) -68 kJ $\mathrm { mol } ^ { - 1 }$ 
C) +39 kJ $\mathrm { mol } ^ { - 1 }$ 
D) -157 kJ $\mathrm { mol } ^ { - 1 }$ 
E) +142 kJ $\mathrm { mol } ^ { - 1 }$

Question 3

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔSsurr at 298 K.Predict whether or not this reaction will be spontaneous at this temperature. 
$\quad$$\quad$N2(g)+ 2O2(g)→ 2NO2(g)ΔrH = +66.4 kJ

Accepted Answer

A) ΔSsurr = +223 J K-1 mol-1,reaction is spontaneous 
B) ΔSsurr = -223J K-1 mol-1,reaction is not spontaneous 
C) ΔSsurr = -66.4 J K-1 mol-1,reaction is spontaneous 
D) ΔSsurr = +66.4 kJ K-1 mol-1,reaction is not spontaneous 
E) ΔSsurr = -66.4 J K-1 mol-1,reaction is not spontaneous 
A) ΔSsurr = +223 J K-1 mol-1,reaction is spontaneous 
B) ΔSsurr = -223J K-1 mol-1,reaction is not spontaneous 
C) ΔSsurr = -66.4 J K-1 mol-1,reaction is spontaneous 
D) ΔSsurr = +66.4 kJ K-1 mol-1,reaction is not spontaneous 
E) ΔSsurr = -66.4 J K-1 mol-1,reaction is not spontaneous

Question 4

Calculate ΔrG° at 298 K using the following information:
$\quad$$\quad$$\quad$ $\quad$$\quad$2HNO3(aq)+ NO(g)→ 3NO2(g)+ H2O(l)$\quad$ΔrG° = ?
ΔfH° (kJ mol-1)-207.0 $\quad$91.3 $\quad$$\quad$33.2 $\quad$$\quad$-285.8
S°(J K-1 mol-1)146.0 $\quad$210.8 $\quad$$\quad$240.1 $\quad$$\quad$70.0

Accepted Answer

A) -151 kJ mol-1 
B) -85.5 kJ mol-1 
C) +50.8 kJ mol-1 
D) +222 kJ mol-1 
E) -186 kJ mol-1 
A) -151 kJ mol-1 
B) -85.5 kJ mol-1 
C) +50.8 kJ mol-1 
D) +222 kJ mol-1 
E) -186 kJ mol-1

Question 5

Give the standard states for a gas,liquid,solid,and solution.

Accepted Answer

For a gas,1 atm; for a liquid,

Question 6

For the following example,what is true about ΔrH and ΔrS? 
$\quad$$\quad$$\quad$3O2(g)→ 2O3(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 7

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

Question 8

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

Accepted Answer

A) This reaction will be spontaneous only at low 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 low temperatures. 
E) This reaction will be spontaneous only at absolute zero (0 Kelvin). 
A) This reaction will be spontaneous only at low 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 low temperatures. 
E) This reaction will be spontaneous only at absolute zero (0 Kelvin).

Question 9

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 10

Above what temperature does the following reaction become nonspontaneous? 
$\quad$$\quad$FeO(s)+ CO(g)→ CO2(g)+ Fe(s)$\quad$ΔrH = -11.0 kJ; ΔrS = -17.4 J K-1 mol-1

Accepted Answer

A) 632 K 
B) 298 K 
C) 191 K 
D) 6.32 × 103 K 
E) 0 K 
A) 632 K 
B) 298 K 
C) 191 K 
D) 6.32 × 103 K 
E) 0 K

Question 11

Determine ΔrG° at 298 K using the following information: 
$\quad$H2(g)+ CO(g)→ CH2O(g)$\quad$ΔrH°= +1.9 kJ mol-1; $\quad$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 12

Place the following in order of decreasing molar entropy at 298 K. 
$\quad$H2 $\quad$Cl2 $\quad$F2

Accepted Answer

A) H2 > Cl2 > F2 
B) Cl2 > H2 > F2 
C) F2 > Cl2 > H2 
D) H2 > F2 > Cl2 
E) Cl2 > F2 > H2 
A) H2 > Cl2 > F2 
B) Cl2 > H2 > F2 
C) F2 > Cl2 > H2 
D) H2 > F2 > Cl2 
E) Cl2 > F2 > H2

Question 13

Identify the statement that is TRUE.

Accepted Answer

A) The entropy of a gas is lower than the entropy of a liquid. 
B) Entropy generally decreases with increasing molecular complexity. 
C) Free atoms have lower entropy than molecules. 
D) Entropy decreases with dissolution. 
E) For noble gases,entropy decreases with increase in atomic size. 
A) The entropy of a gas is lower than the entropy of a liquid. 
B) Entropy generally decreases with increasing molecular complexity. 
C) Free atoms have lower entropy than molecules. 
D) Entropy decreases with dissolution. 
E) For noble gases,entropy decreases with increase in atomic size.

Question 14

Which of the following reactions will have the largest equilibrium constant (K)at 298 K?

Accepted Answer

A) CaCO3(s)→ CaO(s)+ CO2(g)$\quad$$\quad$$\quad$$\quad$$\quad$ ΔrG° =+131.1 kJ mol-1 
B) 2 Hg(g)+ O2(g)→ 2HgO(s)$\quad$$\quad$$\quad$$\quad$ $\quad$$\quad$ΔrG° = -180.8 kJ mol-1 
C) 3O2(g)→ 2O3(g)$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$  ΔrG° = +326 kJ mol-1 
D) Fe2O3(s)+ 3CO(g)→ 2Fe(s)+ 3CO2(g)$\quad$$\quad$ΔrG° = -28.0 kJ mol-1 
A) CaCO3(s)→ CaO(s)+ CO2(g)$\quad$$\quad$$\quad$$\quad$$\quad$ ΔrG° =+131.1 kJ mol-1 
B) 2 Hg(g)+ O2(g)→ 2HgO(s)$\quad$$\quad$$\quad$$\quad$ $\quad$$\quad$ΔrG° = -180.8 kJ mol-1 
C) 3O2(g)→ 2O3(g)$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$  ΔrG° = +326 kJ mol-1 
D) Fe2O3(s)+ 3CO(g)→ 2Fe(s)+ 3CO2(g)$\quad$$\quad$ΔrG° = -28.0 kJ mol-1

Question 15

Choose the statement below that is TRUE.

Accepted Answer

A) If K > 1,ΔrG for forward reaction is positive. 
B) If K rG for forward reaction is negative. 
C) If K > 1,ΔrG for reverse reaction is negative. 
D) ΔrG = 0 at equilibrium. 
E) If K rG for reverse reaction is positive. 
A) If K > 1,ΔrG for forward reaction is positive. 
B) If K rG for forward reaction is negative. 
C) If K > 1,ΔrG for reverse reaction is negative. 
D) ΔrG = 0 at equilibrium. 
E) If K rG for reverse reaction is positive.

Question 16

For the following example,what is true about ΔrH and ΔrS? 
$\quad$$\quad$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 17

The value of ?fG° at 161.0 °C for the formation of phosphorus trichloride from its constituent elements, $P _ { 2 }$ (g)+ $\mathrm { 3Cl } _ { 2 }$ (g)? $2 \mathrm { PCl } _ { 3 }$ (g) is ________ kJ mol-1.At 25.0 °C for this reaction,?fH° is -720.5 kJ mol-1 and $\Delta _ { \mathrm { f } } S ^ { \circ }$ is $- 263.7 \mathrm {~J} \mathrm {~K} ^ { - 1 } \mathrm {~mol} ^ { - 1 }$ .

Accepted Answer

A) -678.0 
B) -834.9 
C) 1.14 × 105 
D) 4.17 × 104 
E) -606.1 
A) -678.0 
B) -834.9 
C) 1.14 × 105 
D) 4.17 × 104 
E) -606.1

Question 18

Define the third law of thermodynamics.

Accepted Answer

The entropy of a per

Question 19

Which of the following is TRUE if ln K is zero?

Accepted Answer

A) ΔrG° is positive and the reaction is spontaneous in the forward direction. 
B) ΔrG° is negative and the reaction is spontaneous in the forward direction. 
C) ΔrG° is negative and the reaction is spontaneous in the reverse direction. 
D) ΔrG° is positive and the reaction is spontaneous in the reverse direction. 
E) ΔrG° is zero and the reaction is at equilibrium. 
A) ΔrG° is positive and the reaction is spontaneous in the forward direction. 
B) ΔrG° is negative and the reaction is spontaneous in the forward direction. 
C) ΔrG° is negative and the reaction is spontaneous in the reverse direction. 
D) ΔrG° is positive and the reaction is spontaneous in the reverse direction. 
E) ΔrG° is zero and the reaction is at equilibrium.

Question 20

Place the following in order of decreasing molar entropy at 298 K. 
HCl $\quad$N2H4 $\quad$Ar

Accepted Answer

A) Ar > N2H4 > HCl 
B) Ar > HCl > N2H4 
C) N2H4 > Ar > HCl 
D) N2H4 > HCl > Ar 
E) HCl > N2H4 > Ar 
A) Ar > N2H4 > HCl 
B) Ar > HCl > N2H4 
C) N2H4 > Ar > HCl 
D) N2H4 > HCl > Ar 
E) HCl > N2H4 > Ar

Exam 17: Gibbs Energy and Thermodynamics

Which of the following statements is TRUE?

Use the following thermodynamic values to calculate ?r G0G ^ { 0 }G0 . Δr\Delta_{r}Δr​H∘ H^{\circ} H∘ = -95 kJ mol−1\mathrm { mol } ^ { - 1 }mol−1 , Δr\Delta_{r}Δr​S0S ^ { 0 }S0 = -157 J mol−1\mathrm { mol } ^ { - 1 }mol−1 ,T = 855 K

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔSsurr at 298 K.Predict whether or not this reaction will be spontaneous at this temperature. \quad\quad N2(g)+ 2O2(g)→ 2NO2(g)ΔrH = +66.4 kJ

Calculate ΔrG° at 298 K using the following information: \quad\quad\quad \quad\quad 2HNO3(aq)+ NO(g)→ 3NO2(g)+ H2O(l) \quad ΔrG° = ? ΔfH° (kJ mol-1)-207.0 \quad 91.3 \quad\quad 33.2 \quad\quad -285.8 S°(J K-1 mol-1)146.0 \quad 210.8 \quad\quad 240.1 \quad\quad 70.0

Give the standard states for a gas,liquid,solid,and solution.

For the following example,what is true about ΔrH and ΔrS? \quad\quad\quad 3O2(g)→ 2O3(g)

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

Consider a reaction that has a negative ΔrH and a negative 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?

Above what temperature does the following reaction become nonspontaneous? \quad\quad FeO(s)+ CO(g)→ CO2(g)+ Fe(s) \quad ΔrH = -11.0 kJ; ΔrS = -17.4 J K-1 mol-1

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

Place the following in order of decreasing molar entropy at 298 K. \quad H2 \quad Cl2 \quad F2

Identify the statement that is TRUE.

Which of the following reactions will have the largest equilibrium constant (K)at 298 K?

Choose the statement below that is TRUE.

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

Define the third law of thermodynamics.

Which of the following is TRUE if ln K is zero?

Place the following in order of decreasing molar entropy at 298 K. HCl \quad N2H4 \quad Ar

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

Use the following thermodynamic values to calculate ?_r $G ^ { 0 }$ . $\Delta_{r}$ $H^{\circ}$ = -95 kJ $\mathrm { mol } ^ { - 1 }$ , $\Delta_{r}$ $S ^ { 0 }$ = -157 J $\mathrm { mol } ^ { - 1 }$ ,T = 855 K

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔS_surrat 298 K.Predict whether or not this reaction will be spontaneous at this temperature. $\quad$ $\quad$ N₂(g)+ 2O₂(g)→ 2NO₂(g)Δ_rH = +66.4 kJ

For the following example,what is true about Δ_rH and Δ_rS? $\quad$ $\quad$ $\quad$ 3O₂(g)→ 2O₃(g)

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

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

Above what temperature does the following reaction become nonspontaneous? $\quad$ $\quad$ FeO(s)+ CO(g)→ CO₂(g)+ Fe(s) $\quad$ Δ_rH = -11.0 kJ; Δ_rS = -17.4 J K^-1 mol^-1

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

Place the following in order of decreasing molar entropy at 298 K. $\quad$ H₂ $\quad$ Cl₂ $\quad$ F₂

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

Place the following in order of decreasing molar entropy at 298 K. HCl $\quad$ N₂H₄ $\quad$ Ar