Consider the following reaction: Ni(CO)4(g) → Ni(s)+ 4CO(g) If the initial concentration of Ni(CO)4(g)is 1.0 M,and x is the equilibrium concentration of CO(g),what is the correct equilibrium relation?

A) Kc = X4/(1.0 - 4X) B) Kc = X/(1.0 - X/4) C) Kc = X4/(1.0 - X/4) D) Kc = X5/(1.0 - X/4) E) Kc = 4X/(1.0 -4X) A) Kc = X4/(1.0 - 4X) B) Kc = X/(1.0 - X/4) C) Kc = X4/(1.0 - X/4) D) Kc = X5/(1.0 - X/4) E) Kc = 4X/(1.0 -4X)

Consider the reaction PCl5(g) →PCl3(g)+ Cl2(g) At a certain temperature,if the initial concentration of PCl5(g)is 2.0 M,at equilibrium the concentration of Cl2(g)is 0.30 M.Calculate the value of Kc at this temperature.

A) 0.064 B) 0.053 C) 0.090 D) 19 E) 0.045 A) 0.064 B) 0.053 C) 0.090 D) 19 E) 0.045

Consider the following reaction at a certain temperature: PCl5(g) →PCl3(g)+ Cl2(g) Kc = 0.100 At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl5(g),PCl3(g),and Cl2(g)is added,what is the equilibrium concentration of PCl5(g)?

A) 0.65 M B) 4.35 M C) 1.35 M D) essentially zero E) 2.35 M A) 0.65 M B) 4.35 M C) 1.35 M D) essentially zero E) 2.35 M

The equilibrium constant for the reaction HNO2(aq)+ H2O(l) →NO2$\rightarrow$(aq)+ H3O+(aq) is 4.3 * 10-4 at 25S1U1P1$\circ$S1S1P0C.Will nitrous acid spontaneously dissociate when [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0 * 10-5 M? Show your calculations.

The answer of The equilibrium constant for the reaction HNO2(aq)+ H2O(l)...

Given: 2SO2(g)+ O2(g) →2SO3(g) At equilibrium at a certain temperature,the concentrations of SO3(g),SO2(g),and O2(g)are 0.24 M,0.82 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

A) 0.89 B) 0.21 C) 0.79 D) 0.26 E) 1.04 A) 0.89 B) 0.21 C) 0.79 D) 0.26 E) 1.04

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 50 bar at this temperature?

A) 2.68 kJ B) 25.2 kJ C) 54.4 kJ D) 16.3 kJ E) -54.4 kJ A) 2.68 kJ B) 25.2 kJ C) 54.4 kJ D) 16.3 kJ E) -54.4 kJ

Consider the reaction PCl5(g) →PCl3(g)+ Cl2(g) At a certain temperature,if the initial concentration of PCl5(g)is 3.0 M,at equilibrium the concentration of Cl2(g)is 0.80 M.Calculate the value of Kc at this temperature.

A) 0.21 B) 0.29 C) 0.64 D) 3.4 E) 0.46 A) 0.21 B) 0.29 C) 0.64 D) 3.4 E) 0.46

Consider the reaction CO(g)+ 2H2(g) →CH3OH(g) At room temperature,K is approximately 2 * 104,but at a higher temperature K is substantially smaller.Which of the following is true?

A) The reaction is endothermic. B) The value of Kc for this reaction is smaller at all temperatures. C) At the higher temperature,more CH3OH(g)is produced. D) The reaction is exothermic. E) The reaction becomes spontaneous at higher temperatures. A) The reaction is endothermic. B) The value of Kc for this reaction is smaller at all temperatures. C) At the higher temperature,more CH3OH(g)is produced. D) The reaction is exothermic. E) The reaction becomes spontaneous at higher temperatures.

Given: SO2(g) →O2(g)+ S(s) Kc = 2.5 * 10-53 SO3(g) → O2(g)+ SO2(g) Kc = 4.0 * 10-13 Calculate Kc for the reaction 2S(s)+ 3O2(g) →2SO3(g)

A) 1.6 * 10103 B) 1.6 * 1080 C) 1.0 *10130 D) 1.6 * 1040 E) 1.0 * 1065 A) 1.6 * 10103 B) 1.6 * 1080 C) 1.0 *10130 D) 1.6 * 1040 E) 1.0 * 1065

Consider the reaction 2Fe2O3(s)+ 3C(s)$\rightarrow$ 4Fe(s)+ 3CO2(g),$\Delta$HS1U1P1$\circ$S1S1P0= 462 kJ,$\Delta$SS1U1P1$\circ$S1S1P0= 558 J.K-1 Calculate the equilibrium constant for this reaction at 525S1U1P1$\circ$S1S1P0C.

A) 3.04 * 10-3 B) 8.07 * 10-2 C) 5.20 * 10-7 D) 1.9 * 106 E) 2.18 * 10-2 A) 3.04 * 10-3 B) 8.07 * 10-2 C) 5.20 * 10-7 D) 1.9 * 106 E) 2.18 * 10-2

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 NH3(g)?

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

At 25S1U1P1$\circ$S1S1P0C,Kc = 1.58 * 10-8 for the reaction NH4(NH2CO2)(s)b 2NH3(g)+ CO2(g) Calculate K at 25S1U1P1$\circ$S1S1P0C for this reaction.

A) 3.87 * 10-7 B) 2.31 * 10-4 C) 9.45 * 10-5 D) 5.69 * 10-3 E) 1.36 * 10-7 A) 3.87 * 10-7 B) 2.31 * 10-4 C) 9.45 * 10-5 D) 5.69 * 10-3 E) 1.36 * 10-7

Exam 11: Chemical Equilibria

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

(Short Answer)

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Question 41

Calculate the vapor pressure of ethyl alcohol,C₂H₅OH(l),at 298 K.The standard free energies of formation of C₂H₅OH(l)and C₂H₅OH(g)are -174.8 and -168.6 kJ.mol^-1,respectively.

(Multiple Choice)

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Question 42

Which of the following reactions is not affected by an increase in pressure?

(Multiple Choice)

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Question 43

Consider the following reaction: Ni(CO)₄(g) → Ni(s)+ 4CO(g) If the initial concentration of Ni(CO)₄(g)is 1.0 M,and x is the equilibrium concentration of CO(g),what is the correct equilibrium relation?

(Multiple Choice)

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Question 44

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 2.0 M,at equilibrium the concentration of Cl₂(g)is 0.30 M.Calculate the value of K_c at this temperature.

(Multiple Choice)

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Question 45

Consider the following reaction at a certain temperature: PCl₅(g) →PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₅(g),PCl₃(g),and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?

(Multiple Choice)

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Question 46

The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) →NO₂ $\rightarrow$ (aq)+ H₃O⁺(aq) is 4.3 * 10^-4 at 25^$\circ$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-5 M? Show your calculations.

(Short Answer)

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Question 47

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.24 M,0.82 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

(Multiple Choice)

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Question 48

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 50 bar at this temperature?

(Multiple Choice)

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Question 49

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 3.0 M,at equilibrium the concentration of Cl₂(g)is 0.80 M.Calculate the value of K_c at this temperature.

(Multiple Choice)

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Question 50

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) →Ni(CO)₄(g) Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.

(Short Answer)

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Question 51

If a 1-L flask containing D₂(g),N₂(g),and ND₃(g)at equilibrium at 300 K and a 1-L flask of H₂(g),N₂(g),and NH₃(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD₂(g),and NH₂D(g)are also present.What conclusion(s)can be drawn?

(Short Answer)

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Question 52

Consider the reaction CO(g)+ 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

(Multiple Choice)

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Question 53

Given: SO₂(g) →O₂(g)+ S(s) K_c = 2.5 * 10^-53 SO₃(g) → O₂(g)+ SO₂(g) K_c = 4.0 * 10^-13 Calculate K_c for the reaction 2S(s)+ 3O₂(g) →2SO₃(g)

(Multiple Choice)

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Question 54

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

(True/False)

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Question 55

Consider the reaction 2Fe₂O₃(s)+ 3C(s) $\rightarrow$ 4Fe(s)+ 3CO₂(g), $\Delta$ H^$\circ$= 462 kJ, $\Delta$ S^$\circ$= 558 J.K^-1 Calculate the equilibrium constant for this reaction at 525^$\circ$C.

(Multiple Choice)

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Question 56

If $\Delta$ G_r^o = 27.1 kJ∙mol^-1 at 25^$\circ$C for the dissociation of acetic acid in aqueous solution,what is K for the reaction CH₃COO^-(aq)+ H₃O⁺(aq) → CH₃COOH(aq)+ H₂O(l)

(Short Answer)

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Question 57

The equilibrium constant expression for the reaction CuSO₄(s) → CuO(s)+ SO₃(g) is K = [CuO(s)][SO₃(g)]/[CuSO₄(s)].

(True/False)

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Question 58

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 NH₃(g)?

(Multiple Choice)

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Question 59

At 25^$\circ$C,K_c = 1.58 * 10^-8 for the reaction NH₄(NH₂CO₂)(s)b 2NH₃(g)+ CO₂(g) Calculate K at 25^$\circ$C for this reaction.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 94

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Calculate the vapor pressure of ethyl alcohol,C₂H₅OH(l),at 298 K.The standard free energies of formation of C₂H₅OH(l)and C₂H₅OH(g)are -174.8 and -168.6 kJ.mol^-1,respectively.

Which of the following reactions is not affected by an increase in pressure?

Consider the following reaction: Ni(CO)₄(g) → Ni(s)+ 4CO(g) If the initial concentration of Ni(CO)₄(g)is 1.0 M,and x is the equilibrium concentration of CO(g),what is the correct equilibrium relation?

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 2.0 M,at equilibrium the concentration of Cl₂(g)is 0.30 M.Calculate the value of K_c at this temperature.

Consider the following reaction at a certain temperature: PCl₅(g) →PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₅(g),PCl₃(g),and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?

The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) →NO₂ $\rightarrow$ (aq)+ H₃O⁺(aq) is 4.3 * 10^-4 at 25^$\circ$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-5 M? Show your calculations.

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.24 M,0.82 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

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 50 bar at this temperature?

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 3.0 M,at equilibrium the concentration of Cl₂(g)is 0.80 M.Calculate the value of K_c at this temperature.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) →Ni(CO)₄(g) Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.

If a 1-L flask containing D₂(g),N₂(g),and ND₃(g)at equilibrium at 300 K and a 1-L flask of H₂(g),N₂(g),and NH₃(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD₂(g),and NH₂D(g)are also present.What conclusion(s)can be drawn?

Consider the reaction CO(g)+ 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

Given: SO₂(g) →O₂(g)+ S(s) K_c = 2.5 * 10^-53 SO₃(g) → O₂(g)+ SO₂(g) K_c = 4.0 * 10^-13 Calculate K_c for the reaction 2S(s)+ 3O₂(g) →2SO₃(g)

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction 2Fe₂O₃(s)+ 3C(s) $\rightarrow$ 4Fe(s)+ 3CO₂(g), $\Delta$ H^$\circ$= 462 kJ, $\Delta$ S^$\circ$= 558 J.K^-1 Calculate the equilibrium constant for this reaction at 525^$\circ$C.

If $\Delta$ G_r^o = 27.1 kJ∙mol^-1 at 25^$\circ$C for the dissociation of acetic acid in aqueous solution,what is K for the reaction CH₃COO^-(aq)+ H₃O⁺(aq) → CH₃COOH(aq)+ H₂O(l)

The equilibrium constant expression for the reaction CuSO₄(s) → CuO(s)+ SO₃(g) is K = [CuO(s)][SO₃(g)]/[CuSO₄(s)].

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 NH₃(g)?

At 25^$\circ$C,K_c = 1.58 * 10^-8 for the reaction NH₄(NH₂CO₂)(s)b 2NH₃(g)+ CO₂(g) Calculate K at 25^$\circ$C for this reaction.

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Exam 11: Chemical Equilibria

For the reaction 2NOCl(g) → 2NO(g)+ Cl2(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl2(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Calculate the vapor pressure of ethyl alcohol,C2H5OH(l),at 298 K.The standard free energies of formation of C2H5OH(l)and C2H5OH(g)are -174.8 and -168.6 kJ.mol-1,respectively.

Which of the following reactions is not affected by an increase in pressure?

Consider the following reaction: Ni(CO)4(g) → Ni(s)+ 4CO(g) If the initial concentration of Ni(CO)4(g)is 1.0 M,and x is the equilibrium concentration of CO(g),what is the correct equilibrium relation?

Consider the reaction PCl5(g) →PCl3(g)+ Cl2(g) At a certain temperature,if the initial concentration of PCl5(g)is 2.0 M,at equilibrium the concentration of Cl2(g)is 0.30 M.Calculate the value of Kc at this temperature.

Consider the following reaction at a certain temperature: PCl5(g) →PCl3(g)+ Cl2(g) Kc = 0.100 At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl5(g),PCl3(g),and Cl2(g)is added,what is the equilibrium concentration of PCl5(g)?

The equilibrium constant for the reaction HNO2(aq)+ H2O(l) →NO2 →\rightarrow→ (aq)+ H3O+(aq) is 4.3 * 10-4 at 25 ∘\circ∘ C.Will nitrous acid spontaneously dissociate when [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0 * 10-5 M? Show your calculations.

Given: 2SO2(g)+ O2(g) →2SO3(g) At equilibrium at a certain temperature,the concentrations of SO3(g),SO2(g),and O2(g)are 0.24 M,0.82 M,and 0.33 M,respectively.Calculate the value of Kc for this reaction.

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 50 bar at this temperature?

Consider the reaction PCl5(g) →PCl3(g)+ Cl2(g) At a certain temperature,if the initial concentration of PCl5(g)is 3.0 M,at equilibrium the concentration of Cl2(g)is 0.80 M.Calculate the value of Kc at this temperature.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) →Ni(CO)4(g) Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)4(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.

If a 1-L flask containing D2(g),N2(g),and ND3(g)at equilibrium at 300 K and a 1-L flask of H2(g),N2(g),and NH3(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD2(g),and NH2D(g)are also present.What conclusion(s)can be drawn?

Consider the reaction CO(g)+ 2H2(g) →CH3OH(g) At room temperature,K is approximately 2 * 104,but at a higher temperature K is substantially smaller.Which of the following is true?

Given: SO2(g) →O2(g)+ S(s) Kc = 2.5 * 10-53 SO3(g) → O2(g)+ SO2(g) Kc = 4.0 * 10-13 Calculate Kc for the reaction 2S(s)+ 3O2(g) →2SO3(g)

Consider the following N2O4(g) →2NO2(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction 2Fe2O3(s)+ 3C(s) →\rightarrow→ 4Fe(s)+ 3CO2(g), Δ\DeltaΔ H ∘\circ∘ = 462 kJ, Δ\DeltaΔ S ∘\circ∘ = 558 J.K-1 Calculate the equilibrium constant for this reaction at 525 ∘\circ∘ C.

If Δ\DeltaΔ Gro = 27.1 kJ∙mol-1 at 25 ∘\circ∘ C for the dissociation of acetic acid in aqueous solution,what is K for the reaction CH3COO-(aq)+ H3O+(aq) → CH3COOH(aq)+ H2O(l)

The equilibrium constant expression for the reaction CuSO4(s) → CuO(s)+ SO3(g) is K = [CuO(s)][SO3(g)]/[CuSO4(s)].

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 NH3(g)?

At 25 ∘\circ∘ C,Kc = 1.58 * 10-8 for the reaction NH4(NH2CO2)(s)b 2NH3(g)+ CO2(g) Calculate K at 25 ∘\circ∘ C for this reaction.

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Aqueous Equilibria

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For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Calculate the vapor pressure of ethyl alcohol,C₂H₅OH(l),at 298 K.The standard free energies of formation of C₂H₅OH(l)and C₂H₅OH(g)are -174.8 and -168.6 kJ.mol^-1,respectively.

Consider the following reaction: Ni(CO)₄(g) → Ni(s)+ 4CO(g) If the initial concentration of Ni(CO)₄(g)is 1.0 M,and x is the equilibrium concentration of CO(g),what is the correct equilibrium relation?

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 2.0 M,at equilibrium the concentration of Cl₂(g)is 0.30 M.Calculate the value of K_c at this temperature.

Consider the following reaction at a certain temperature: PCl₅(g) →PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₅(g),PCl₃(g),and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?

The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) →NO₂ $\rightarrow$ (aq)+ H₃O⁺(aq) is 4.3 * 10^-4 at 25^$\circ$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-5 M? Show your calculations.

Given: 2SO₂(g)+ O₂(g) →2SO₃(g) At equilibrium at a certain temperature,the concentrations of SO₃(g),SO₂(g),and O₂(g)are 0.24 M,0.82 M,and 0.33 M,respectively.Calculate the value of K_c for this reaction.

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 50 bar at this temperature?

Consider the reaction PCl₅(g) →PCl₃(g)+ Cl₂(g) At a certain temperature,if the initial concentration of PCl₅(g)is 3.0 M,at equilibrium the concentration of Cl₂(g)is 0.80 M.Calculate the value of K_c at this temperature.

Consider the following reaction at a certain temperature: Ni(s)+ 4CO(g) →Ni(CO)₄(g) Calculate K for this reaction if,at equilibrium,the partial pressures of CO(g)and Ni(CO)₄(g)are 1.25 and 6.65 atm over 1.00 kg of nickel.

If a 1-L flask containing D₂(g),N₂(g),and ND₃(g)at equilibrium at 300 K and a 1-L flask of H₂(g),N₂(g),and NH₃(g)at equilibrium at 300 K are mixed,analysis of the reaction mixture shows that HD(g),NHD₂(g),and NH₂D(g)are also present.What conclusion(s)can be drawn?

Consider the reaction CO(g)+ 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

Given: SO₂(g) →O₂(g)+ S(s) K_c = 2.5 * 10^-53 SO₃(g) → O₂(g)+ SO₂(g) K_c = 4.0 * 10^-13 Calculate K_c for the reaction 2S(s)+ 3O₂(g) →2SO₃(g)

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction 2Fe₂O₃(s)+ 3C(s) $\rightarrow$ 4Fe(s)+ 3CO₂(g), $\Delta$ H^$\circ$= 462 kJ, $\Delta$ S^$\circ$= 558 J.K^-1 Calculate the equilibrium constant for this reaction at 525^$\circ$C.

If $\Delta$ G_r^o = 27.1 kJ∙mol^-1 at 25^$\circ$C for the dissociation of acetic acid in aqueous solution,what is K for the reaction CH₃COO^-(aq)+ H₃O⁺(aq) → CH₃COOH(aq)+ H₂O(l)

The equilibrium constant expression for the reaction CuSO₄(s) → CuO(s)+ SO₃(g) is K = [CuO(s)][SO₃(g)]/[CuSO₄(s)].

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 NH₃(g)?

At 25^$\circ$C,K_c = 1.58 * 10^-8 for the reaction NH₄(NH₂CO₂)(s)b 2NH₃(g)+ CO₂(g) Calculate K at 25^$\circ$C for this reaction.