Consider the reaction CuSO4(s)$\rightarrow$ CuO(s)+ SO3(g) If $\Delta$GS1U1P1$\circ$S1S1P0 = -14.6 kJ at 950S1U1P1$\circ$S1S1P0C for this reaction,what is $\Delta$G for an SO3(g)pressure of 20 bar at this temperature.

A) 15.9 kJ B) 45.1 kJ C) -14.6 kJ D) 30.5 kJ E) -45.1 kJ A) 15.9 kJ B) 45.1 kJ C) -14.6 kJ D) 30.5 kJ E) -45.1 kJ A

Calculate $\Delta$G at 298 K for the reaction C2H5OH(l)$\rightarrow$ C2H5OH(g,0.0400 bar) Given $\Delta$GS1U1P1$\circ$S1S1P0 = 6.2 kJ at 298 K.

A) 14 kJ B) 2.7 kJ C) -14 kJ D) -1.8 kJ E) 1.8 kJ A) 14 kJ B) 2.7 kJ C) -14 kJ D) -1.8 kJ E) 1.8 kJ

The equilibrium constant K for the dissociation of N2O4(g)to NO2(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction,$\Delta$HS1U1P1$\circ$S1S1P0 is 56.8 kJ.mol-1.

A) 1.32 * 10-6 B) 1.11 * 10-4 C) 15.5 D) 0.188 E) 1.54 * 107 A) 1.32 * 10-6 B) 1.11 * 10-4 C) 15.5 D) 0.188 E) 1.54 * 107

At 25S1U1P1$\circ$S1S1P0C,Kc = 4.1 * 108 for the reaction N2(g)+ 3H2(g) →2NH3(g) Calculate K at 25S1U1P1$\circ$S1S1P0C for this reaction.

A) 9.7 * 107 B) 6.9 * 105 C) 4.1 * 108 D) 1.7 * 109 E) 2.5 * 1011 A) 9.7 * 107 B) 6.9 * 105 C) 4.1 * 108 D) 1.7 * 109 E) 2.5 * 1011

Consider the reaction 3Fe(s)+ 4H2O(g) → 4H2(g)+ Fe3O4(s) If the volume of the container is reduced,

A) the equilibrium constant increases. B) more H2(g)is produced. C) no change occurs. D) more H2O(g)is produced. E) more Fe(s)is produced. A) the equilibrium constant increases. B) more H2(g)is produced. C) no change occurs. D) more H2O(g)is produced. E) more Fe(s)is produced.

Given: 2SO2(g)+ O2(g) →2SO3(g) At equilibrium at a certain temperature,the concentrations of SO3(g),SO2(g),and O2(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

A) 1.31 B) 0.42 C) 0.014 D) 0.059 E) 0.87 A) 1.31 B) 0.42 C) 0.014 D) 0.059 E) 0.87

For the reaction NH3(g)+ H2S(g) →NH4HS(s) Kc = 9.7 at 900 K.If the initial concentrations of NH3(g)and H2S(g)are 2.0 M,what is the equilibrium concentration of H2S(g)?

A) 1.9 M B) 0.20 M C) 1.7 M D) 0.10 M E) 0.32 M A) 1.9 M B) 0.20 M C) 1.7 M D) 0.10 M E) 0.32 M

If $\Delta$GS1U1P1$\circ$S1S1P0= 27.1 kJ at 25S1U1P1$\circ$S1S1P0C for the reaction CH3COOH(aq)+ H2O(l) → CH3COO-(aq)+ H3O+(aq) What is Ka for this reaction at 298 K?

A) 1.15 *10-11 B) 5.63 * 104 C) 1.78 * 10-5 D) 1.01 E) 9.89 * 10-1 A) 1.15 *10-11 B) 5.63 * 104 C) 1.78 * 10-5 D) 1.01 E) 9.89 * 10-1

Consider the reaction NO(g)+ O2(g)$\rightarrow$ NO2(g) If $\Delta$HS1U1P1$\circ$S1S1P0 = -56.52 kJ and $\Delta$SS1U1P1$\circ$S1S1P0 = -72.60 J.K-1 at 298 K,what is the equilibrium constant for the reaction at 298 K?

A) 1.31 * 106 B) 7.63 * 10-7 C) 660 D) 1.22 * 1014 E) 8.08 * 109 A) 1.31 * 106 B) 7.63 * 10-7 C) 660 D) 1.22 * 1014 E) 8.08 * 109

What is the relation between K and Kc for the reaction H2(g)+ I2(g) →2HI(g)

A) K = Kc B) K = RTKc C) Kc = (RT)2K D) K = (RT)2Kc E) Kc = RTK A) K = Kc B) K = RTKc C) Kc = (RT)2K D) K = (RT)2Kc E) Kc = RTK

At 25S1U1P1$\circ$S1S1P0C,$\Delta$GS1U1B1rS1U1B0S1U1P1oS1S1P0 for the reaction 2SOS1U1B12S1U1B0(g)+ OS1U1B12S1U1B0(g) ?S1U1B02SOS1U1B13S1U1B0(g)is -141.74 kJ·molS1U1P1-1S1S1P0.Calculate the value of KS1U1B1cS1U1B0 for this reaction.

A) 1.74 * 10S1U1P126S1S1P0 B) 7.01 * 10S1U1P124S1S1P0 C) 2.65 * 10S1U1P112S1S1P0 D) 6.56 * 10S1U1P113S1S1P0 A) 1.74 * 10S1U1P126S1S1P0 B) 7.01 * 10S1U1P124S1S1P0 C) 2.65 * 10S1U1P112S1S1P0 D) 6.56 * 10S1U1P113S1S1P0

Calculate the value of K at 700 K for the reaction H2(g)+ I2(g) → 2HI(g) Given that Kc = 54 at the same temperature.

A) 3100 B) 2.2 C) 54 D) 9.3 E) 1300 A) 3100 B) 2.2 C) 54 D) 9.3 E) 1300

Exam 11: Chemical Equilibria

Calculate the standard free energy of formation of chloroform,CHCl₃(l),at 25°C.The standard free energy of formation of CHCl₃(g)is -70.12 kJ.mol^-1 and the vapor pressure of chloroform at 25°C is 0.499 atm.

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Question 1

Correct Answer:

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-71.84 kJ.mol^-1

Consider the reaction CuSO₄(s) $\rightarrow$ CuO(s)+ SO₃(g) If $\Delta$ G^$\circ$ = -14.6 kJ at 950^$\circ$C for this reaction,what is $\Delta$ G for an SO₃(g)pressure of 20 bar at this temperature.

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Question 2

Correct Answer:

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Given: 4NH₃(g)+ 5O₂(g) → 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NH₃(g)+ O₂(g) →2NO(g)+ 3H₂O(g)

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Question 3

Correct Answer:

Verified

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0400 bar) Given $\Delta$ G^$\circ$ = 6.2 kJ at 298 K.

(Multiple Choice)

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Question 4

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g)concentration?

(Multiple Choice)

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Question 5

The equilibrium constant K for the dissociation of N₂O₄(g)to NO₂(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction, $\Delta$ H^$\circ$ is 56.8 kJ.mol^-1.

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Question 6

Consider the reaction 2SO₂(g)+ O₂(g) $\leftrightarrow$ 2SO₃(g) At equilibrium at a certain temperature,the partial pressures of SO₂(g),O₂(g),and SO₃(g)are 0.0012,0.18,and 2.2 bar,respectively.Argon is introduced into the reaction vessel until the partial pressure of argon is 5.0 bar.Predict the final partial pressures of the reactants and products.

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Question 7

At 25^$\circ$C,K_c = 4.1 * 10⁸ for the reaction N₂(g)+ 3H₂(g) →2NH₃(g) Calculate K at 25^$\circ$C for this reaction.

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Question 8

Consider the reaction 3Fe(s)+ 4H₂O(g) → 4H₂(g)+ Fe₃O₄(s) If the volume of the container is reduced,

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Question 9

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

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Question 10

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

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Question 11

For the reaction NH₃(g)+ H₂S(g) →NH₄HS(s) K_c = 9.7 at 900 K.If the initial concentrations of NH₃(g)and H₂S(g)are 2.0 M,what is the equilibrium concentration of H₂S(g)?

(Multiple Choice)

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Question 12

If $\Delta$ G^$\circ$= 27.1 kJ at 25^$\circ$C for the reaction CH₃COOH(aq)+ H₂O(l) → CH₃COO^-(aq)+ H₃O⁺(aq) What is K_a for this reaction at 298 K?

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Question 13

Consider the reaction CO₂(g)+ C(s)→ 2CO(g) At equilibrium,at a certain temperature,the partial pressures of CO₂(g)and CO(g)are 23.5 and 8.21 atm,respectively.Calculate the value of K_P.

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Question 14

Consider the reaction NO(g)+ $Consider the reaction NO(g)+ O2(g) \rightarrow NO2(g) If \Delta H \circ = -56.52 kJ and \Delta S \circ = -72.60 J.K-1 at 298 K,what is the equilibrium constant for the reaction at 298 K?$ O₂(g) $\rightarrow$ NO₂(g) If $\Delta$ H^$\circ$ = -56.52 kJ and $\Delta$ S^$\circ$ = -72.60 J.K^-1 at 298 K,what is the equilibrium constant for the reaction at 298 K?

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Question 15

Given: P₄(s)+ 6Cl₂(g)b 4PCl₃(l) K Calculate the equilibrium constant for the following reaction. 2PCl₃(l) →3Cl₂(g)+ P₄(s)

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Question 16

What is the relation between K and K_c for the reaction H₂(g)+ I₂(g) →2HI(g)

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Question 17

At 25^$\circ$C, $\Delta$ G_r^o for the reaction 2SO₂(g)+ O₂(g) ?2SO₃(g)is -141.74 kJ·mol^-1.Calculate the value of K_c for this reaction.

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Question 18

Calculate the value of K at 700 K for the reaction H₂(g)+ I₂(g) → 2HI(g) Given that K_c = 54 at the same temperature.

(Multiple Choice)

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Question 19

What is the relationship between K and K_c for the reaction below? N₂(g)+ 3H₂(g) →2NH₃(g)

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Question 20

Showing 1 - 20 of 94

Calculate the standard free energy of formation of chloroform,CHCl₃(l),at 25°C.The standard free energy of formation of CHCl₃(g)is -70.12 kJ.mol^-1 and the vapor pressure of chloroform at 25°C is 0.499 atm.

Consider the reaction CuSO₄(s) $\rightarrow$ CuO(s)+ SO₃(g) If $\Delta$ G^$\circ$ = -14.6 kJ at 950^$\circ$C for this reaction,what is $\Delta$ G for an SO₃(g)pressure of 20 bar at this temperature.

Given: 4NH₃(g)+ 5O₂(g) → 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NH₃(g)+ O₂(g) →2NO(g)+ 3H₂O(g)

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0400 bar) Given $\Delta$ G^$\circ$ = 6.2 kJ at 298 K.

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g)concentration?

The equilibrium constant K for the dissociation of N₂O₄(g)to NO₂(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction, $\Delta$ H^$\circ$ is 56.8 kJ.mol^-1.

At 25^$\circ$C,K_c = 4.1 * 10⁸ for the reaction N₂(g)+ 3H₂(g) →2NH₃(g) Calculate K at 25^$\circ$C for this reaction.

Consider the reaction 3Fe(s)+ 4H₂O(g) → 4H₂(g)+ Fe₃O₄(s) If the volume of the container is reduced,

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

For the reaction NH₃(g)+ H₂S(g) →NH₄HS(s) K_c = 9.7 at 900 K.If the initial concentrations of NH₃(g)and H₂S(g)are 2.0 M,what is the equilibrium concentration of H₂S(g)?

If $\Delta$ G^$\circ$= 27.1 kJ at 25^$\circ$C for the reaction CH₃COOH(aq)+ H₂O(l) → CH₃COO^-(aq)+ H₃O⁺(aq) What is K_a for this reaction at 298 K?

Consider the reaction CO₂(g)+ C(s)→ 2CO(g) At equilibrium,at a certain temperature,the partial pressures of CO₂(g)and CO(g)are 23.5 and 8.21 atm,respectively.Calculate the value of K_P.

Given: P₄(s)+ 6Cl₂(g)b 4PCl₃(l) K Calculate the equilibrium constant for the following reaction. 2PCl₃(l) →3Cl₂(g)+ P₄(s)

What is the relation between K and K_c for the reaction H₂(g)+ I₂(g) →2HI(g)

At 25^$\circ$C, $\Delta$ G_r^o for the reaction 2SO₂(g)+ O₂(g) ?2SO₃(g)is -141.74 kJ·mol^-1.Calculate the value of K_c for this reaction.

Calculate the value of K at 700 K for the reaction H₂(g)+ I₂(g) → 2HI(g) Given that K_c = 54 at the same temperature.

What is the relationship between K and K_c for the reaction below? N₂(g)+ 3H₂(g) →2NH₃(g)

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Exam 11: Chemical Equilibria

Calculate the standard free energy of formation of chloroform,CHCl3(l),at 25°C.The standard free energy of formation of CHCl3(g)is -70.12 kJ.mol-1 and the vapor pressure of chloroform at 25°C is 0.499 atm.

Consider the reaction CuSO4(s) →\rightarrow→ CuO(s)+ SO3(g) If Δ\DeltaΔ G ∘\circ∘ = -14.6 kJ at 950 ∘\circ∘ C for this reaction,what is Δ\DeltaΔ G for an SO3(g)pressure of 20 bar at this temperature.

Given: 4NH3(g)+ 5O2(g) → 4NO(g)+ 6H2O(g) K Calculate the equilibrium constant for the following reaction. 2NH3(g)+ O2(g) →2NO(g)+ 3H2O(g)

Calculate Δ\DeltaΔ G at 298 K for the reaction C2H5OH(l) →\rightarrow→ C2H5OH(g,0.0400 bar) Given Δ\DeltaΔ G ∘\circ∘ = 6.2 kJ at 298 K.

For the reaction N2O4(g) →2NO2(g) Which of the following disturbances will cause an increase in NO2(g)concentration?

The equilibrium constant K for the dissociation of N2O4(g)to NO2(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction, Δ\DeltaΔ H ∘\circ∘ is 56.8 kJ.mol-1.

At 25 ∘\circ∘ C,Kc = 4.1 * 108 for the reaction N2(g)+ 3H2(g) →2NH3(g) Calculate K at 25 ∘\circ∘ C for this reaction.

Consider the reaction 3Fe(s)+ 4H2O(g) → 4H2(g)+ Fe3O4(s) If the volume of the container is reduced,

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)4(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)4(g) → Ni(s)+ 4CO(g)

Given: 2SO2(g)+ O2(g) →2SO3(g) At equilibrium at a certain temperature,the concentrations of SO3(g),SO2(g),and O2(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

For the reaction NH3(g)+ H2S(g) →NH4HS(s) Kc = 9.7 at 900 K.If the initial concentrations of NH3(g)and H2S(g)are 2.0 M,what is the equilibrium concentration of H2S(g)?

If Δ\DeltaΔ G ∘\circ∘ = 27.1 kJ at 25 ∘\circ∘ C for the reaction CH3COOH(aq)+ H2O(l) → CH3COO-(aq)+ H3O+(aq) What is Ka for this reaction at 298 K?

Consider the reaction CO2(g)+ C(s)→ 2CO(g) At equilibrium,at a certain temperature,the partial pressures of CO2(g)and CO(g)are 23.5 and 8.21 atm,respectively.Calculate the value of KP.

Consider the reaction NO(g)+ O2(g) →\rightarrow→ NO2(g) If Δ\DeltaΔ H ∘\circ∘ = -56.52 kJ and Δ\DeltaΔ S ∘\circ∘ = -72.60 J.K-1 at 298 K,what is the equilibrium constant for the reaction at 298 K?

Given: P4(s)+ 6Cl2(g)b 4PCl3(l) K Calculate the equilibrium constant for the following reaction. 2PCl3(l) →3Cl2(g)+ P4(s)

What is the relation between K and Kc for the reaction H2(g)+ I2(g) →2HI(g)

At 25 ∘\circ∘ C, Δ\DeltaΔ Gro for the reaction 2SO2(g)+ O2(g) ?2SO3(g)is -141.74 kJ·mol-1.Calculate the value of Kc for this reaction.

Calculate the value of K at 700 K for the reaction H2(g)+ I2(g) → 2HI(g) Given that Kc = 54 at the same temperature.

What is the relationship between K and Kc for the reaction below? N2(g)+ 3H2(g) →2NH3(g)

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Calculate the standard free energy of formation of chloroform,CHCl₃(l),at 25°C.The standard free energy of formation of CHCl₃(g)is -70.12 kJ.mol^-1 and the vapor pressure of chloroform at 25°C is 0.499 atm.

Consider the reaction CuSO₄(s) $\rightarrow$ CuO(s)+ SO₃(g) If $\Delta$ G^$\circ$ = -14.6 kJ at 950^$\circ$C for this reaction,what is $\Delta$ G for an SO₃(g)pressure of 20 bar at this temperature.

Given: 4NH₃(g)+ 5O₂(g) → 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NH₃(g)+ O₂(g) →2NO(g)+ 3H₂O(g)

Calculate $\Delta$ G at 298 K for the reaction C₂H₅OH(l) $\rightarrow$ C₂H₅OH(g,0.0400 bar) Given $\Delta$ G^$\circ$ = 6.2 kJ at 298 K.

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g)concentration?

The equilibrium constant K for the dissociation of N₂O₄(g)to NO₂(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction, $\Delta$ H^$\circ$ is 56.8 kJ.mol^-1.

At 25^$\circ$C,K_c = 4.1 * 10⁸ for the reaction N₂(g)+ 3H₂(g) →2NH₃(g) Calculate K at 25^$\circ$C for this reaction.

Consider the reaction 3Fe(s)+ 4H₂O(g) → 4H₂(g)+ Fe₃O₄(s) If the volume of the container is reduced,

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.12 M,0.86 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

For the reaction NH₃(g)+ H₂S(g) →NH₄HS(s) K_c = 9.7 at 900 K.If the initial concentrations of NH₃(g)and H₂S(g)are 2.0 M,what is the equilibrium concentration of H₂S(g)?

If $\Delta$ G^$\circ$= 27.1 kJ at 25^$\circ$C for the reaction CH₃COOH(aq)+ H₂O(l) → CH₃COO^-(aq)+ H₃O⁺(aq) What is K_a for this reaction at 298 K?

Consider the reaction CO₂(g)+ C(s)→ 2CO(g) At equilibrium,at a certain temperature,the partial pressures of CO₂(g)and CO(g)are 23.5 and 8.21 atm,respectively.Calculate the value of K_P.

Given: P₄(s)+ 6Cl₂(g)b 4PCl₃(l) K Calculate the equilibrium constant for the following reaction. 2PCl₃(l) →3Cl₂(g)+ P₄(s)

What is the relation between K and K_c for the reaction H₂(g)+ I₂(g) →2HI(g)

At 25^$\circ$C, $\Delta$ G_r^o for the reaction 2SO₂(g)+ O₂(g) ?2SO₃(g)is -141.74 kJ·mol^-1.Calculate the value of K_c for this reaction.

Calculate the value of K at 700 K for the reaction H₂(g)+ I₂(g) → 2HI(g) Given that K_c = 54 at the same temperature.

What is the relationship between K and K_c for the reaction below? N₂(g)+ 3H₂(g) →2NH₃(g)