Question 1

How many microstates are possible in a collection of four particles that are present, with two particles each in two connected flasks?

Accepted Answer

six or 6 or six microstates or 6 microstates

Question 2

For a given reaction, ΔrH = +35.5 kJ mol-1 and ΔrS = +83.6 J K-1 mol-1. The reaction is spontaneous ________. Assume that ΔrH and ΔrS do not vary with temperature.

Accepted Answer

A) at T 298 K C) at all temperatures D) at T > 425 K E) at T < 298 K A) at T 298 K C) at all temperatures D) at T > 425 K E) at T < 298 K D

Question 3

Which of the following statements is TRUE?

Accepted Answer

A)  Entropy is an extensive property. 
B)  Entropy is not temperature dependent. 
C)  Exothermic processes decrease the entropy of the surroundings. 
D)  ΔSuniv is always greater than zero for a nonspontaneous process. 
E)  Just like enthalpy, entropy has no absolute zero value. 
A)  Entropy is an extensive property. 
B)  Entropy is not temperature dependent. 
C)  Exothermic processes decrease the entropy of the surroundings. 
D)  ΔSuniv is always greater than zero for a nonspontaneous process. 
E)  Just like enthalpy, entropy has no absolute zero value. A

Question 4

Determine ΔrG° at 298 K using the following information: CaCO3(s) → CaO(s) + CO2(g) ΔrH°= +179.2 kJ mol-1; ΔrS°= +160.2 J K-1 mol-1

Accepted Answer

A)  -607.0 kJ mol-1 
B)  +112 .0 kJ mol-1 
C)  -89.3 kJ mol-1 
D)  +131.5 kJ mol-1 
E)  +228.1 kJ mol-1 
A)  -607.0 kJ mol-1 
B)  +112 .0 kJ mol-1 
C)  -89.3 kJ mol-1 
D)  +131.5 kJ mol-1 
E)  +228.1 kJ mol-1

Question 5

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔrG° = -23.0 kJ mol-1
Calculate ΔrG° for the following reaction:
9NO(g) → 3N2O(g) + 3NO2(g)

Accepted Answer

A)  -23.0 kJ mol-1 
B)  69.0 kJ mol-1 
C)  -69.0 kJ mol-1 
D)  -7.67 kJ mol-1 
E)  23.0 kJ mol-1 
A)  -23.0 kJ mol-1 
B)  69.0 kJ mol-1 
C)  -69.0 kJ mol-1 
D)  -7.67 kJ mol-1 
E)  23.0 kJ mol-1

Question 6

For the following example, what is true about ΔrH and ΔrS? H2O(l) → H2O(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

Which of the following processes have a ΔrS > 0?

Accepted Answer

A)  2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) 
B)  lithium fluoride forms from Li and F2 
C)  2HBr(g) → H2(g) + Br2(l) 
D)  sodium chloride dissolves in pure water 
E)  Ag+(aq) + Cl-(aq) → AgCl(s) 
A)  2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) 
B)  lithium fluoride forms from Li and F2 
C)  2HBr(g) → H2(g) + Br2(l) 
D)  sodium chloride dissolves in pure water 
E)  Ag+(aq) + Cl-(aq) → AgCl(s)

Question 8

Estimate ΔrG° for the following reaction at 449.0 K. CH2O(g) + 2H2(g) → CH4(g) + H2O(g) ΔrH°= -94.9 kJ mol-1; ΔrS°= -224.2 J K-1 mol-1

Accepted Answer

A)  +5.8 kJ mol-1 
B)  +12.9 kJ mol-1 
C)  -101 kJ mol-1 
D)  +2.4 kJ mol-1 
E)  -4.2 kJ mol-1 
A)  +5.8 kJ mol-1 
B)  +12.9 kJ mol-1 
C)  -101 kJ mol-1 
D)  +2.4 kJ mol-1 
E)  -4.2 kJ mol-1

Question 9

Define allotrope.

Accepted Answer

An allotrope is two

Question 10

Consider the following reaction at constant pressure. Use the information here to determine the value of ?SS1U1B1surr S1U1B0at 355 K. Predict whether or not this reaction will be spontaneous at this temperature. 2NO(g) + OS1U1B12S1U1B0(g) ? 2NOS1U1B12S1U1B0(g) ?S1U1B1rS1U1B0H = -114 kJ

Accepted Answer

A)  ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is spontaneous 
B)  ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous 
C)  ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is spontaneous 
D)  ?SS1U1B1surrS1U1B0 = -321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous 
E)  ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous 
A)  ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is spontaneous 
B)  ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous 
C)  ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is spontaneous 
D)  ?SS1U1B1surrS1U1B0 = -321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous 
E)  ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0, reaction is not spontaneous

Question 11

Place the following in order of decreasing standard molar entropy. N2O4 NO NO2

Accepted Answer

A)  N2O4 > NO2 > NO 
B)  NO > NO2 > N2O4 
C)  N2O4 > NO > NO2 
D)  NO > N2O4 > NO2 
E)  NO2 > NO > N2O4 
A)  N2O4 > NO2 > NO 
B)  NO > NO2 > N2O4 
C)  N2O4 > NO > NO2 
D)  NO > N2O4 > NO2 
E)  NO2 > NO > N2O4

Question 12

Use Hess's law to calculate ΔrG° using the following information: ClO(g) + O3(g) → Cl(g) + 2O2(g) ΔrG° = ?
2O3(g)→ 3O2(g) ΔrG° = +489.6 kJ mol-1
Cl(g) + O3(g) → ClO(g) + O2(g) ΔrG° = -34.5 kJ mol-1

Accepted Answer

A)  -472.4 kJ mol-1 
B)  -210.3 kJ mol-1 
C)  +455.1 kJ mol-1 
D)  +262.1 kJ mol-1 
E)  +524.1 kJ mol-1 
A)  -472.4 kJ mol-1 
B)  -210.3 kJ mol-1 
C)  +455.1 kJ mol-1 
D)  +262.1 kJ mol-1 
E)  +524.1 kJ mol-1

Question 13

Identify the compound with the lowest standard Gibbs energy of formation.

Accepted Answer

A)  NaCl(s) 
B)  N2(g) 
C)  NO(g) 
D)  O3(g) 
E)  Cl2(g) 
A)  NaCl(s) 
B)  N2(g) 
C)  NO(g) 
D)  O3(g) 
E)  Cl2(g)

Question 14

Use the following thermodynamic values to calculate Δr     .
Δr
    = -95 kJ   , Δr
    = -157 J   , T = 298 K

Accepted Answer

A)  -48 kJ   
B)  -68 kJ   
C)  + 39 kJ   
D)  -157 kJ   
E)  +142 kJ   
A)  -48 kJ   
B)  -68 kJ   
C)  + 39 kJ   
D)  -157 kJ   
E)  +142 kJ

Question 15

What is the name of the reaction that achieves 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 16

Determine ΔrG° at 298 K using the following information: N2(g) + O2(g) → 2NO(g) ΔrH°= +182.6 kJ mol-1; ΔrS°= +24.8 J K-1 mol-1

Accepted Answer

A)  -607.0 kJ mol-1 
B)  +68.4 .0 kJ mol-1 
C)  -89.3 kJ mol-1 
D)  +131.5 kJ mol-1 
E)  +175.2 kJ mol-1 
A)  -607.0 kJ mol-1 
B)  +68.4 .0 kJ mol-1 
C)  -89.3 kJ mol-1 
D)  +131.5 kJ mol-1 
E)  +175.2 kJ mol-1

Question 17

Calculate ΔrS° for the following reaction. The S° for each species is shown below the reaction. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
S°(J K-1 mol-1) 192.8 205.2 210.8 188.8

Accepted Answer

A)  +287.4 J K-1 mol-1 
B)  -401.2 J K-1 mol-1 
C)  +160.0 J K-1 mol-1 
D)  -336.6 J K-1 mol-1 
E)  +178.8 J K-1 mol-1 
A)  +287.4 J K-1 mol-1 
B)  -401.2 J K-1 mol-1 
C)  +160.0 J K-1 mol-1 
D)  -336.6 J K-1 mol-1 
E)  +178.8 J K-1 mol-1

Question 18

Use the following thermodynamic values to calculate Δr     .
Δr
    = +95 kJ   , Δr
    = -157 J   , T = 398 K

Accepted Answer

A)  -48 kJ   
B)  -68 kJ   
C)  +39 kJ   
D)  +157 kJ   
E)  +142 kJ   
A)  -48 kJ   
B)  -68 kJ   
C)  +39 kJ   
D)  +157 kJ   
E)  +142 kJ

Question 19

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

Question 20

Calculate ΔrG° at 298 K using the following information: 2HNO3(aq) + NO(g) → 3NO2(g) + H2O(l) ΔrG° = ?
ΔfG° (kJ mol-1) -110.9 87.6 51.3 -237.1

Accepted Answer

A)  -162.5 kJ mol-1 
B)  +51.0 kJ mol-1 
C)  -54.5 kJ mol-1 
D)  +171.1 kJ mol-1 
E)  -87.6 kJ mol-1 
A)  -162.5 kJ mol-1 
B)  +51.0 kJ mol-1 
C)  -54.5 kJ mol-1 
D)  +171.1 kJ mol-1 
E)  -87.6 kJ mol-1

Exam 17: Gibbs Energy and Thermodynamics

How many microstates are possible in a collection of four particles that are present, with two particles each in two connected flasks?

For a given reaction, ΔrH = +35.5 kJ mol-1 and ΔrS = +83.6 J K-1 mol-1. The reaction is spontaneous ________. Assume that ΔrH and ΔrS do not vary with temperature.

Which of the following statements is TRUE?

Determine ΔrG° at 298 K using the following information: CaCO3(s) → CaO(s) + CO2(g) ΔrH°= +179.2 kJ mol-1; ΔrS°= +160.2 J K-1 mol-1

Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔrG° = -23.0 kJ mol-1 Calculate ΔrG° for the following reaction: 9NO(g) → 3N2O(g) + 3NO2(g)

For the following example, what is true about ΔrH and ΔrS? H2O(l) → H2O(g)

Which of the following processes have a ΔrS > 0?

Estimate ΔrG° for the following reaction at 449.0 K. CH2O(g) + 2H2(g) → CH4(g) + H2O(g) ΔrH°= -94.9 kJ mol-1; ΔrS°= -224.2 J K-1 mol-1

Define allotrope.

Consider the following reaction at constant pressure. Use the information here to determine the value of ?Ssurr at 355 K. Predict whether or not this reaction will be spontaneous at this temperature. 2NO(g) + O2(g) ? 2NO2(g) ?rH = -114 kJ

Place the following in order of decreasing standard molar entropy. N2O4 NO NO2

Use Hess's law to calculate ΔrG° using the following information: ClO(g) + O3(g) → Cl(g) + 2O2(g) ΔrG° = ? 2O3(g)→ 3O2(g) ΔrG° = +489.6 kJ mol-1 Cl(g) + O3(g) → ClO(g) + O2(g) ΔrG° = -34.5 kJ mol-1

Identify the compound with the lowest standard Gibbs energy of formation.

Use the following thermodynamic values to calculate Δr . Δr = -95 kJ , Δr = -157 J , T = 298 K

What is the name of the reaction that achieves the theoretical limits with respect to the change in Gibbs energy in thermodynamics?

Determine ΔrG° at 298 K using the following information: N2(g) + O2(g) → 2NO(g) ΔrH°= +182.6 kJ mol-1; ΔrS°= +24.8 J K-1 mol-1

Calculate ΔrS° for the following reaction. The S° for each species is shown below the reaction. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) S°(J K-1 mol-1) 192.8 205.2 210.8 188.8

Use the following thermodynamic values to calculate Δr . Δr = +95 kJ , Δr = -157 J , T = 398 K

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

Calculate ΔrG° at 298 K using the following information: 2HNO3(aq) + NO(g) → 3NO2(g) + H2O(l) ΔrG° = ? ΔfG° (kJ mol-1) -110.9 87.6 51.3 -237.1

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For a given reaction, Δ_rH = +35.5 kJ mol^-1 and Δ_rS = +83.6 J K^-1mol^-1. The reaction is spontaneous ________. Assume that Δ_rH and Δ_rS do not vary with temperature.

Determine Δ_rG° at 298 K using the following information: CaCO₃(s) → CaO(s) + CO₂(g) Δ_rH°= +179.2 kJ mol^-1; Δ_rS°= +160.2 J K^-1 mol^-¹

Given the following equation, N₂O(g) + NO₂(g) → 3 NO(g) Δ_rG° = -23.0 kJ mol^-1 Calculate Δ_rG° for the following reaction: 9NO(g) → 3N₂O(g) + 3NO₂(g)

For the following example, what is true about Δ_rH and Δ_rS? H₂O(l) → H₂O(g)

Which of the following processes have a Δ_rS > 0?

Estimate Δ_rG° for the following reaction at 449.0 K. CH₂O(g) + 2H₂(g) → CH₄(g) + H₂O(g) Δ_rH°= -94.9 kJ mol^-1; Δ_rS°= -224.2 J K^-1 mol^-1

Consider the following reaction at constant pressure. Use the information here to determine the value of ?S_surrat 355 K. Predict whether or not this reaction will be spontaneous at this temperature. 2NO(g) + O₂(g) ? 2NO₂(g) ?_rH = -114 kJ

Place the following in order of decreasing standard molar entropy. N₂O₄ NO NO₂

Use Hess's law to calculate Δ_rG°using the following information: ClO(g) + O₃(g) → Cl(g) + 2O₂(g) Δ_rG°= ? 2O₃(g)→ 3O₂(g) Δ_rG°= +489.6 kJ mol^-1 Cl(g) + O₃(g) → ClO(g) + O₂(g) Δ_rG°= -34.5 kJ mol^-1

Use the following thermodynamic values to calculate Δ_r . Δ_r = -95 kJ , Δ_r = -157 J , T = 298 K

Determine Δ_rG° at 298 K using the following information: N₂(g) + O₂(g) → 2NO(g) Δ_rH°= +182.6 kJ mol^-1; Δ_rS°= +24.8 J K^-1 mol^-1

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g) S°(J K^-1 mol^-1) 192.8 205.2 210.8 188.8

Use the following thermodynamic values to calculate Δ_r . Δ_r = +95 kJ , Δ_r = -157 J , T = 398 K

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

Calculate Δ_rG° at 298 K using the following information: 2HNO₃(aq) + NO(g) → 3NO₂(g) + H₂O(l) Δ_rG°= ? Δ_fG° (kJ mol^-1) -110.9 87.6 51.3 -237.1