Below what temperature does the following reaction become nonspontaneous? 2HNO3(aq)+ NO(g)→ 3NO2(g)+ H2O(l)ΔrH = +136.5 kJ; ΔrS = +287.5 J K-1 mol-1

A) 39.2 K B) 151 K C) 475 K D) 4.75 × 103 K E) 298.17 K A) 39.2 K B) 151 K C) 475 K D) 4.75 × 103 K E) 298.17 K

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

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

Calculate ΔrG at 298 K under the conditions shown below for the following reaction: 2Hg(g)+ O2(g)→ 2HgO(s) ΔG° = -180.8 kJ mol-1 P(Hg)= 0.025 atm, P(O2)= 0.037 atm

A) +207 kJ mol-1 B) -154.4 kJ mol-1 C) -26.5 kJ mol-1 D) -164 kJ mol-1 E) +60.7 kJ mol-1 A) +207 kJ mol-1 B) -154.4 kJ mol-1 C) -26.5 kJ mol-1 D) -164 kJ mol-1 E) +60.7 kJ mol-1

The value of ΔfG° at 100.0 °C for the formation of calcium chloride from its constituent elements, Ca(s)+ Cl2(g) → CaCl2(s) Is __________ kJ mol-1. At 25.0 °C for this reaction, ΔfH° is -795.8 kJ mol-1l, ΔfG° is -748.1 kJ mol-1, and ΔfS° is -159.8 J K-1 mol-1.

A) -855.4 B) -736.2 C) 5.88 × 104 D) -779.8 E) 1.52 × 104 A) -855.4 B) -736.2 C) 5.88 × 104 D) -779.8 E) 1.52 × 104

Use Hess's law to calculate ΔrG° using the following information: CO(g)→ C(s)+ 1/2 O2(g) ΔrG° = ? CO2(g)→ C(s)+ O2(g)ΔrG° = +394.4 kJ mol-1 CO(g)+ 1/2 O2(g)→ CO2(g)ΔrG° = -257.2 kJ mol-1

A) -60.0 kJ mol-1 B) +651.6 kJ mol-1 C) -265.8 kJ mol-1 D) +137.2 kJ mol-1 E) +523.0 kJ mol-1 A) -60.0 kJ mol-1 B) +651.6 kJ mol-1 C) -265.8 kJ mol-1 D) +137.2 kJ mol-1 E) +523.0 kJ mol-1

Calculate ?S1U1B1rS1U1B0G° at 298 K using the following information: 2HNOS1U1B13S1U1B0(aq)+ NO(g)? 3NOS1U1B12S1U1B0(g)+ HS1U1B12S1U1B0O(l)?S1U1B1rS1U1B0G° = ? ?S1U1B1fS1U1B0H° (kJ molS1U1P1-1S1S1P0)-207.0 91.3 33.2 -285.8 S°(J KS1U1P1-1S1S1P0 molS1U1P1-1S1S1P0)146.0 210.8 240.1 70.0

A) -151 kJ molS1U1P1-1S1S1P0 B) -85.5 kJ molS1U1P1-1S1S1P0 C) +50.8 kJ molS1U1P1-1S1S1P0 D) +222 kJ molS1U1P1-1S1S1P0 E) -186 kJ molS1U1P1-1S1S1P0 A) -151 kJ molS1U1P1-1S1S1P0 B) -85.5 kJ molS1U1P1-1S1S1P0 C) +50.8 kJ molS1U1P1-1S1S1P0 D) +222 kJ molS1U1P1-1S1S1P0 E) -186 kJ molS1U1P1-1S1S1P0

Determine the equilibrium constant for the following reaction at 298 K: SO3(g)+ H2O(g)→ H2SO4(l)ΔrG° = -90.5 kJ mol-1

A) 1.37 × 10-16 B) 4.78 × 1011 C) 9.11 × 10-8 D) 7.31 × 1015 E) 0.964 A) 1.37 × 10-16 B) 4.78 × 1011 C) 9.11 × 10-8 D) 7.31 × 1015 E) 0.964

Exam 17: Gibbs Energy and Thermodynamics

Below what temperature does the following reaction become nonspontaneous? 2HNO₃(aq)+ NO(g)→ 3NO₂(g)+ H₂O(l)Δ_rH = +136.5 kJ; Δ_rS = +287.5 J K^-1 mol^-1

(Multiple Choice)

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Question 21

What is "free" energy? Give a fictitious example.

(Essay)

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Question 22

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. C₂H₂(g)+ H₂(g)→ C₂H₄(g) S°(J J K^-1 mol^-1)200.9 130.7 219.3

(Multiple Choice)

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Question 23

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

(Multiple Choice)

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Question 24

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: 2Hg(g)+ O₂(g)→ 2HgO(s) ΔG° = -180.8 kJ mol^-1 P(Hg)= 0.025 atm, P(O₂)= 0.037 atm

(Multiple Choice)

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Question 25

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

(Multiple Choice)

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Question 26

Identify the compound with the standard Gibbs energy of formation equal to zero.

(Multiple Choice)

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Question 27

Which of the following processes have a Δ_rS = 0?

(Multiple Choice)

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Question 28

Which of the following processes have a Δ_rS > 0?

(Multiple Choice)

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Question 29

The value of Δ_fG° at 100.0 °C for the formation of calcium chloride from its constituent elements, Ca(s)+ Cl₂(g) → CaCl₂(s) Is __________ kJ mol^-1. At 25.0 °C for this reaction, Δ_fH° is -795.8 kJ mol^-1l, Δ_fG° is -748.1 kJ mol^-1, and Δ_fS° is -159.8 J K^-1 mol^-1.

(Multiple Choice)

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Question 30

Match the following. -Q < 1

(Multiple Choice)

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Question 31

Match the following. -Q = 1

(Multiple Choice)

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Question 32

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

(Essay)

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Question 33

Determine the equilibrium constant for the following reaction at 298 K: Cl(g)+ O₃(g)→ ClO(g)+ O₂(g)Δ_rG° = - 34.5 kJ mol^-1

(Multiple Choice)

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Question 34

Use Hess's law to calculate Δ_rG° using the following information: CO(g)→ C(s)+ 1/2 O₂(g) Δ_rG°= ? CO₂(g)→ C(s)+ O₂(g)Δ_rG°= +394.4 kJ mol^-1 CO(g)+ 1/2 O₂(g)→ CO₂(g)Δ_rG°= -257.2 kJ mol^-1

(Multiple Choice)

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Question 35

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. N₂(g)+ 2O₂(g)→ 2NO₂(g)Δ_rH = +66.4 kJ

(Multiple Choice)

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Question 36

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

(Multiple Choice)

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Question 37

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

(Multiple Choice)

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Question 38

Determine the equilibrium constant for the following reaction at 298 K: SO₃(g)+ H₂O(g)→ H₂SO₄(l)Δ_rG° = -90.5 kJ mol^-1

(Multiple Choice)

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Question 39

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

(Multiple Choice)

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Question 40

Showing 21 - 40 of 111

Exam 17: Gibbs Energy and Thermodynamics

Below what temperature does the following reaction become nonspontaneous? 2HNO3(aq)+ NO(g)→ 3NO2(g)+ H2O(l)ΔrH = +136.5 kJ; ΔrS = +287.5 J K-1 mol-1

What is "free" energy? Give a fictitious example.

Calculate ΔrS° for the following reaction. The S° for each species is shown below the reaction. C2H2(g)+ H2(g)→ C2H4(g) S°(J J K-1 mol-1)200.9 130.7 219.3

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

Calculate ΔrG at 298 K under the conditions shown below for the following reaction: 2Hg(g)+ O2(g)→ 2HgO(s) ΔG° = -180.8 kJ mol-1 P(Hg)= 0.025 atm, P(O2)= 0.037 atm

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

Identify the compound with the standard Gibbs energy of formation equal to zero.

Which of the following processes have a ΔrS = 0?

Which of the following processes have a ΔrS > 0?

The value of ΔfG° at 100.0 °C for the formation of calcium chloride from its constituent elements, Ca(s)+ Cl2(g) → CaCl2(s) Is __________ kJ mol-1. At 25.0 °C for this reaction, ΔfH° is -795.8 kJ mol-1l, ΔfG° is -748.1 kJ mol-1, and ΔfS° is -159.8 J K-1 mol-1.

Match the following. -Q < 1

Match the following. -Q = 1

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

Determine the equilibrium constant for the following reaction at 298 K: Cl(g)+ O3(g)→ ClO(g)+ O2(g)ΔrG° = - 34.5 kJ mol-1

Use Hess's law to calculate ΔrG° using the following information: CO(g)→ C(s)+ 1/2 O2(g) ΔrG° = ? CO2(g)→ C(s)+ O2(g)ΔrG° = +394.4 kJ mol-1 CO(g)+ 1/2 O2(g)→ CO2(g)ΔrG° = -257.2 kJ mol-1

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. N2(g)+ 2O2(g)→ 2NO2(g)ΔrH = +66.4 kJ

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

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

Determine the equilibrium constant for the following reaction at 298 K: SO3(g)+ H2O(g)→ H2SO4(l)ΔrG° = -90.5 kJ mol-1

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

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Below what temperature does the following reaction become nonspontaneous? 2HNO₃(aq)+ NO(g)→ 3NO₂(g)+ H₂O(l)Δ_rH = +136.5 kJ; Δ_rS = +287.5 J K^-1 mol^-1

Calculate Δ_rS° for the following reaction. The S° for each species is shown below the reaction. C₂H₂(g)+ H₂(g)→ C₂H₄(g) S°(J J K^-1 mol^-1)200.9 130.7 219.3

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

Calculate Δ_rG at 298 K under the conditions shown below for the following reaction: 2Hg(g)+ O₂(g)→ 2HgO(s) ΔG° = -180.8 kJ mol^-1 P(Hg)= 0.025 atm, P(O₂)= 0.037 atm

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

Which of the following processes have a Δ_rS = 0?

Which of the following processes have a Δ_rS > 0?

The value of Δ_fG° at 100.0 °C for the formation of calcium chloride from its constituent elements, Ca(s)+ Cl₂(g) → CaCl₂(s) Is __________ kJ mol^-1. At 25.0 °C for this reaction, Δ_fH° is -795.8 kJ mol^-1l, Δ_fG° is -748.1 kJ mol^-1, and Δ_fS° is -159.8 J K^-1 mol^-1.

Determine the equilibrium constant for the following reaction at 298 K: Cl(g)+ O₃(g)→ ClO(g)+ O₂(g)Δ_rG° = - 34.5 kJ mol^-1

Use Hess's law to calculate Δ_rG° using the following information: CO(g)→ C(s)+ 1/2 O₂(g) Δ_rG°= ? CO₂(g)→ C(s)+ O₂(g)Δ_rG°= +394.4 kJ mol^-1 CO(g)+ 1/2 O₂(g)→ CO₂(g)Δ_rG°= -257.2 kJ mol^-1

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. N₂(g)+ 2O₂(g)→ 2NO₂(g)Δ_rH = +66.4 kJ

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

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

Determine the equilibrium constant for the following reaction at 298 K: SO₃(g)+ H₂O(g)→ H₂SO₄(l)Δ_rG° = -90.5 kJ mol^-1

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