Consider the following reaction at constant pressure.Use the information here to determine the value of ?SS1U1B1surrS1U1B0 at 355 K.Predict whether or not this reaction will be spontaneous at this temperature. $\quad$$\quad$$\quad$2NO(g)+ OS1U1B12S1U1B0(g)? 2NOS1U1B12S1U1B0(g)?S1U1B1rS1U1B0H = -114 kJ

A) ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is spontaneous B) ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous C) ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is spontaneous D) ?SS1U1B1surrS1U1B0= -321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous E) ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous A) ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is spontaneous B) ?SS1U1B1surrS1U1B0 = +114 kJ KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous C) ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is spontaneous D) ?SS1U1B1surrS1U1B0= -321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous E) ?SS1U1B1surrS1U1B0 = +321 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0,reaction is not spontaneous

Use Hess's law to calculate ΔrG° using the following information: CO(g)→ C(s)+ 1/2 O2(g)$\quad$$\quad$ΔrG° = ? CO2(g)→ C(s)+ O2(g)$\quad$$\quad$$\quad$ΔrG° = +394.4 kJ mol-1 CO(g)+ 1/2 O2(g)→ CO2(g)$\quad$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 the equilibrium constant for the following reaction at 298 K: 2H2S(g)→ 2H2(g)+ S2(g)$\quad$$\quad$ΔrH° = 169.8 kJ mol-1; ΔrS°= 78.0 J K-1 mol-1

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

Estimate ΔrG° for the following reaction at 775 K. $\quad$$\quad$2Hg(g)+ O2(g)→ 2HgO(s)$\quad$ΔrH°= -304.2 kJ mol-1; $\quad$$\quad$ΔrS°= -414.2 J K-1 mol-1

A) -625 kJ mol-1 B) -181 kJ mol-1 C) +17 kJ mol-1 D) +321 kJ mol-1 E) -110 kJ mol-1 A) -625 kJ mol-1 B) -181 kJ mol-1 C) +17 kJ mol-1 D) +321 kJ mol-1 E) -110 kJ mol-1

Determine the equilibrium constant for the following reaction at 655 K: $\quad$HCN(g)+ 2H2(g)→ CH3NH2(g)ΔrH° = -158 kJ mol-1; $\quad$ΔrS°= -219.9 J K-1 mol-1

A) 3.99 × 1012 B) 13.0 C) 2.51 × 10-13 D) 3.26 × 10-12 E) 3.07 × 1011 A) 3.99 × 1012 B) 13.0 C) 2.51 × 10-13 D) 3.26 × 10-12 E) 3.07 × 1011

Calculate ?S1U1B1rS1U1B0S° for the following reaction.The S°for each species is shown below the reaction. $\quad$$\quad$$\quad$$\quad$$\quad$$\quad$$\quad$CS1U1B12S1U1B0HS1U1B12S1U1B0(g)+ 2HS1U1B12S1U1B0(g)? CS1U1B12S1U1B0HS1U1B16S1U1B0(g) S°(J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0)$\quad$$\quad$$\quad$200.9 $\quad$130.7 $\quad$229.2

A) +303.3 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 B) +560.8 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 C) -102.4 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 D) -233.1 J KS1U1P1-1S1S1P0molS1U1P1-1S1S1P0 E) 229.2 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 A) +303.3 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 B) +560.8 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 C) -102.4 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0 D) -233.1 J KS1U1P1-1S1S1P0molS1U1P1-1S1S1P0 E) 229.2 J KS1U1P1-1 S1S1P0molS1U1P1-1S1S1P0

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

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 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

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

Exam 17: Gibbs Energy and Thermodynamics

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

(Multiple Choice)

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Question 41

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

(Multiple Choice)

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Question 42

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

(Multiple Choice)

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Question 43

What is the change in Gibbs energy of a process?

(Multiple Choice)

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Question 44

Estimate Δ_rG° for the following reaction at 775 K. $\quad$ $\quad$ 2Hg(g)+ O₂(g)→ 2HgO(s) $\quad$ Δ_rH°= -304.2 kJ mol^-1; $\quad$ $\quad$ Δ_rS°= -414.2 J K^-1 mol^-1

(Multiple Choice)

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Question 45

Which of the following statements is TRUE?

(Multiple Choice)

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Question 46

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

(Multiple Choice)

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Question 47

Determine the equilibrium constant for the following reaction at 655 K: $\quad$ HCN(g)+ 2H₂(g)→ CH₃NH₂(g)Δ_rH° = -158 kJ mol^-1; $\quad$ Δ_rS°= -219.9 J K^-1 mol^-1

(Multiple Choice)

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Question 48

Calculate ?_rS° for the following reaction.The S°for each species is shown below the reaction. $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ C₂H₂(g)+ 2H₂(g)? C₂H₆(g) S°(J K^-1mol^-1) $\quad$ $\quad$ $\quad$ 200.9 $\quad$ 130.7 $\quad$ 229.2

(Multiple Choice)

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Question 49

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

(Multiple Choice)

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Question 50

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 = 298 K

(Multiple Choice)

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Question 51

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

(Multiple Choice)

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Question 52

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔS_surr at 398 K.Predict whether or not this reaction will be spontaneous at this temperature. $\quad$ $\quad$ $\quad$ 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(g)Δ_rH = -1267 kJ

(Multiple Choice)

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Question 53

Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25 °C?

(Multiple Choice)

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Question 54

Calculate Δ_rS° for the following reaction.The S° for each species is shown below the reaction. $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ N₂H₄(l)+ H₂(g)→ 2NH₃(g) S° (J K^-1 mol^-1) $\quad$ 121.2 $\quad$ $\quad$ 130.7 $\quad$ 192.8

(Multiple Choice)

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Question 55

Place the following in order of increasing molar entropy at 298 K. $\quad$ NO $\quad$ CO $\quad$ SO

(Multiple Choice)

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Question 56

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

(Multiple Choice)

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Question 57

Calculate ?_rG for the evaporation of methanol at 25°C under nonstandard conditions when $\mathrm { PCH } _ { 3 } \mathrm { OH }$ = 150.0 mbar $\quad$ $\quad$ $\quad$ CH₃OH(l)? CH₃OH(g)

(Multiple Choice)

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Question 58

Which one of the following has the highest standard molar entropy,S°,at 25 °C?

(Multiple Choice)

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Question 59

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

(Multiple Choice)

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Question 60

Showing 41 - 60 of 119

Exam 17: Gibbs Energy and Thermodynamics

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. \quad\quad\quad 2NO(g)+ O2(g)? 2NO2(g)?rH = -114 kJ

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

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

What is the change in Gibbs energy of a process?

Estimate ΔrG° for the following reaction at 775 K. \quad\quad 2Hg(g)+ O2(g)→ 2HgO(s) \quad ΔrH°= -304.2 kJ mol-1; \quad\quad ΔrS°= -414.2 J K-1 mol-1

Which of the following statements is TRUE?

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

Determine the equilibrium constant for the following reaction at 655 K: \quad HCN(g)+ 2H2(g)→ CH3NH2(g)ΔrH° = -158 kJ mol-1; \quad ΔrS°= -219.9 J K-1 mol-1

Calculate ?rS° for the following reaction.The S°for each species is shown below the reaction. \quad\quad\quad\quad\quad\quad\quad C2H2(g)+ 2H2(g)? C2H6(g) S°(J K-1 mol-1) \quad\quad\quad 200.9 \quad 130.7 \quad 229.2

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

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 = 298 K

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

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔSsurr at 398 K.Predict whether or not this reaction will be spontaneous at this temperature. \quad\quad\quad 4NH3(g)+ 3O2(g)→ 2N2(g)+ 6H2O(g)ΔrH = -1267 kJ

Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25 °C?

Calculate ΔrS° for the following reaction.The S° for each species is shown below the reaction. \quad\quad\quad\quad\quad\quad\quad N2H4(l)+ H2(g)→ 2NH3(g) S° (J K-1 mol-1) \quad 121.2 \quad\quad 130.7 \quad 192.8

Place the following in order of increasing molar entropy at 298 K. \quad NO \quad CO \quad SO

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

Calculate ?rG for the evaporation of methanol at 25°C under nonstandard conditions when PCH3OH\mathrm { PCH } _ { 3 } \mathrm { OH }PCH3​OH = 150.0 mbar \quad\quad\quad CH3OH(l)? CH3OH(g)

Which one of the following has the highest standard molar entropy,S°,at 25 °C?

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

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

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

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

Estimate Δ_rG° for the following reaction at 775 K. $\quad$ $\quad$ 2Hg(g)+ O₂(g)→ 2HgO(s) $\quad$ Δ_rH°= -304.2 kJ mol^-1; $\quad$ $\quad$ Δ_rS°= -414.2 J K^-1 mol^-1

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

Determine the equilibrium constant for the following reaction at 655 K: $\quad$ HCN(g)+ 2H₂(g)→ CH₃NH₂(g)Δ_rH° = -158 kJ mol^-1; $\quad$ Δ_rS°= -219.9 J K^-1 mol^-1

Calculate ?_rS° for the following reaction.The S°for each species is shown below the reaction. $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ C₂H₂(g)+ 2H₂(g)? C₂H₆(g) S°(J K^-1mol^-1) $\quad$ $\quad$ $\quad$ 200.9 $\quad$ 130.7 $\quad$ 229.2

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

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 = 298 K

Consider the following reaction at constant pressure.Use the information here to determine the value of ΔS_surr at 398 K.Predict whether or not this reaction will be spontaneous at this temperature. $\quad$ $\quad$ $\quad$ 4NH₃(g)+ 3O₂(g)→ 2N₂(g)+ 6H₂O(g)Δ_rH = -1267 kJ

Calculate Δ_rS° for the following reaction.The S° for each species is shown below the reaction. $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ $\quad$ N₂H₄(l)+ H₂(g)→ 2NH₃(g) S° (J K^-1 mol^-1) $\quad$ 121.2 $\quad$ $\quad$ 130.7 $\quad$ 192.8

Place the following in order of increasing molar entropy at 298 K. $\quad$ NO $\quad$ CO $\quad$ SO

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

Calculate ?_rG for the evaporation of methanol at 25°C under nonstandard conditions when $\mathrm { PCH } _ { 3 } \mathrm { OH }$ = 150.0 mbar $\quad$ $\quad$ $\quad$ CH₃OH(l)? CH₃OH(g)

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