4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction: Br2(l)+ Cl2(g)⇌ 2 BrCl(g) At the point of equilibrium there were 82.63 g of Br2(l).Determine the total pressure in the 50.0 L container at equilibrium.

A) 0.110 atm B) 2.64 atm C) 0.180 atm D) 1.43 atm E) 1.21 atm A) 0.110 atm B) 2.64 atm C) 0.180 atm D) 1.43 atm E) 1.21 atm

For the reaction;N2(g)+ 3 H2(g)⇌ 2 NH3(g),the equilibrium amount of NH3 will be increased by: I.increasing the pressure II.adding H2 III.removing N2 IV.decreasing the pressure

A) I,III B) III only C) II,III D) I,II E) II,IV A) I,III B) III only C) II,III D) I,II E) II,IV

A mixture,containing 0.0750 M HCl(g)and 0.0330 M O2(g)is allowed to come to equilibrium at 480 °C. 4 HCl(g)+ O2(g)⇌ 2 Cl2(g)+ 2 H2O(g) At equilibrium [Cl2] = 0.030 M.What is the value of Kc?

A) 1.1 × 10-3 B) 890 C) 0.13 D) 1.3 E) 480 A) 1.1 × 10-3 B) 890 C) 0.13 D) 1.3 E) 480

For the following reaction O2(g)⇌ 2 O(g) What conditions favor production of oxygen atoms?

A) high temperature and low pressure B) high temperature and high pressure C) low temperature and low pressure D) low temperature and high pressure A) high temperature and low pressure B) high temperature and high pressure C) low temperature and low pressure D) low temperature and high pressure

For the reaction: PCl3(g)+ Cl2(g)⇌ PCl5(g)at 85 °C,Kp = 1.19 If one starts with 2.00 atm pressure of PCl3,1.00 atm pressure of Cl2 and no PCl5,what is the partial pressure of PCl5(g)at equilibrium?

A) 0.167 atm B) 0.739 atm C) 0.621 atm D) 0.465 atm E) 0.553 atm A) 0.167 atm B) 0.739 atm C) 0.621 atm D) 0.465 atm E) 0.553 atm

For CO2(g)+ H2(g)⇌ CO(g)+ H2O(g),Kc = [CO][H2]/[CO2][H2],if there are 1.43 mols each of CO and H2O,0.572 mol H2 and 4.572 mols CO2,in a 4.0 L container at equilibrium,what is Kc?

A) 0.547 B) 0.782 C) 1.28 D) 0.137 E) 2.34 A) 0.547 B) 0.782 C) 1.28 D) 0.137 E) 2.34

For the reaction below CO(g)+ 2 H2(g)⇌ CH3OH(g) The equilibrium concentrations at 483 K are [CO] = 0.0753 M,[H2] = 0.151 M,and [CH3OH] = 0.0247 M.Calculate the value of Kc.

A) 14.4 B) 1.09 C) 2.17 D) 0.0694 E) 0.917 A) 14.4 B) 1.09 C) 2.17 D) 0.0694 E) 0.917

For 2 NO2(g)⇌ N2O4(g),Kc = [N2O4]/[NO2]2.At equilibrium there are 0.0270 mol N2O4 and 0.450 mol NO2 in a 50.0-L container.What is Kc?

A) 0.00267 B) 6.81 C) 6.67 D) 0.133 E) 2.45 A) 0.00267 B) 6.81 C) 6.67 D) 0.133 E) 2.45

Consider the following reaction at a certain temperature. 2 SO3(g)⇌ 2 SO2(g)+ O2(g) When the initial concentration of SO3(g)is 0.128 M,the concentration of oxygen gas at equilibrium is found to be 0.0130 M.Calculate Kc for this reaction.

A) 8.45 × 10-4 B) 1.62 × 10-2 C) 7.64 × 10-5 D) 1.47 × 10-3 A) 8.45 × 10-4 B) 1.62 × 10-2 C) 7.64 × 10-5 D) 1.47 × 10-3

For the reaction: H2(g)+ I2(g)⇌ 2 HI(g),Kc = 92.0 When equilibrium concentrations of HI and I2 are [HI] = 0.115 M and [I2] = 0.250 M,the equilibrium concentration of [H2] is:

A) 5.00 × 10-3 M B) 5.75 × 10-4 M C) 1.74 × 103 M D) 0.135 M E) 9.56 M A) 5.00 × 10-3 M B) 5.75 × 10-4 M C) 1.74 × 103 M D) 0.135 M E) 9.56 M

For the reaction: CH4(g)+ 2 H2O(g)⇌ CO2(g)+ 4 H2(g),ΔrH° = +190 kJ,when the temperature is raised to 1200 K:

A) the reaction shifts to the right B) the reaction shifts to the left C) the ΔrH° increases D) the temperature increases E) there is no change in equilibrium position A) the reaction shifts to the right B) the reaction shifts to the left C) the ΔrH° increases D) the temperature increases E) there is no change in equilibrium position

Consider the following equation: N2O4(g)⇌ 2 NO2(g),Kc = 5.8 × 10-3 If the initial concentration of N2O4(g)= 0.040 M and the initial concentration of NO2(g)is 0 M,what is the equilibrium concentration of N2O4(g)?

A) 1.7 × 10-2 M B) 1.9 × 10-2 M C) 3.3 × 10-2 M D) 2.6 × 10-2 M E) 2.3 × 10-6 M A) 1.7 × 10-2 M B) 1.9 × 10-2 M C) 3.3 × 10-2 M D) 2.6 × 10-2 M E) 2.3 × 10-6 M

Exam 15: Principles of Chemical Equilibrium

Consider the equilibrium system: N₂O₄(g)⇌ 2 NO₂(g)for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

(Multiple Choice)

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Question 101

4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction: Br₂(l)+ Cl₂(g)⇌ 2 BrCl(g) At the point of equilibrium there were 82.63 g of Br₂(l).Determine the total pressure in the 50.0 L container at equilibrium.

(Multiple Choice)

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Question 102

For the reaction;N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g),the equilibrium amount of NH₃ will be increased by: I.increasing the pressure II.adding H₂ III.removing N₂ IV.decreasing the pressure

(Multiple Choice)

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Question 103

Consider the following gas phase reaction at 25 °C. N₂(g)+ C₂H₂(g)⇌ 2 HCN(g) 1.600 mol N₂(g)and 1.750 mol C₂H₂(g)are placed in a 1.000 L vessel and the mixture is allowed to react.At equilibrium,there are 1.587 mol N₂(g)in the mixture.What is K_c for this reaction at 25 °C?

(Multiple Choice)

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Question 104

Write the equilibrium expression K_c for the reaction: Sodium sulfite(aq)+ chloric acid (aq)⇌ sodium chlorate(aq)+ sulfur dioxide(g)+ water(l).

(Multiple Choice)

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Question 105

A mixture,containing 0.0750 M HCl(g)and 0.0330 M O₂(g)is allowed to come to equilibrium at 480 °C. 4 HCl(g)+ O₂(g)⇌ 2 Cl₂(g)+ 2 H₂O(g) At equilibrium [Cl₂] = 0.030 M.What is the value of K_c?

(Multiple Choice)

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Question 106

For the following reaction O₂(g)⇌ 2 O(g) What conditions favor production of oxygen atoms?

(Multiple Choice)

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Question 107

In a reaction at equilibrium involving only gases,a change in pressure of the reaction mixture shifts the position of equilibrium only when:

(Multiple Choice)

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Question 108

For the reaction: PCl₃(g)+ Cl₂(g)⇌ PCl₅(g)at 85 °C,K_p = 1.19 If one starts with 2.00 atm pressure of PCl₃,1.00 atm pressure of Cl₂ and no PCl₅,what is the partial pressure of PCl₅(g)at equilibrium?

(Multiple Choice)

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Question 109

For CO₂(g)+ H₂(g)⇌ CO(g)+ H₂O(g),K_c = [CO][H₂]/[CO₂][H₂],if there are 1.43 mols each of CO and H₂O,0.572 mol H₂ and 4.572 mols CO₂,in a 4.0 L container at equilibrium,what is K_c?

(Multiple Choice)

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Question 110

For the reaction below CO(g)+ 2 H₂(g)⇌ CH₃OH(g) The equilibrium concentrations at 483 K are [CO] = 0.0753 M,[H₂] = 0.151 M,and [CH₃OH] = 0.0247 M.Calculate the value of K_c.

(Multiple Choice)

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Question 111

Changes in temperature cause change in the equilibrium position.

(True/False)

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Question 112

For 2 NO₂(g)⇌ N₂O₄(g),K_c = [N₂O₄]/[NO₂]².At equilibrium there are 0.0270 mol N₂O₄ and 0.450 mol NO₂ in a 50.0-L container.What is K_c?

(Multiple Choice)

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Question 113

Consider the following reaction at a certain temperature. 2 SO₃(g)⇌ 2 SO₂(g)+ O₂(g) When the initial concentration of SO₃(g)is 0.128 M,the concentration of oxygen gas at equilibrium is found to be 0.0130 M.Calculate K_c for this reaction.

(Multiple Choice)

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Question 114

For the reaction: H₂(g)+ I₂(g)⇌ 2 HI(g),K_c = 92.0 When equilibrium concentrations of HI and I₂ are [HI] = 0.115 M and [I₂] = 0.250 M,the equilibrium concentration of [H₂] is:

(Multiple Choice)

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Question 115

What will happen to the equilibrium in the reaction 2 A(g)⇌ B(g)+ C(g),K_c = 1.25 at 300 K,if a catalyst is added?

(Multiple Choice)

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Question 116

For the reaction: CH₄(g)+ 2 H₂O(g)⇌ CO₂(g)+ 4 H₂(g),Δ_rH° = +190 kJ,when the temperature is raised to 1200 K:

(Multiple Choice)

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Question 117

Consider the following equation: N₂O₄(g)⇌ 2 NO₂(g),K_c = 5.8 × 10^-3 If the initial concentration of N₂O₄(g)= 0.040 M and the initial concentration of NO₂(g)is 0 M,what is the equilibrium concentration of N₂O₄(g)?

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Question 118

Showing 101 - 118 of 118

Exam 15: Principles of Chemical Equilibrium

Consider the equilibrium system: N2O4(g)⇌ 2 NO2(g)for which Kp = 0.1134 at 25 °C and ΔrH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container,compute At equilibrium.

4.000 mol chlorine and 2.000 mol bromine were placed in a 50.0 L container and kept at 293 K until equilibrium was achieved for the reaction: Br2(l)+ Cl2(g)⇌ 2 BrCl(g) At the point of equilibrium there were 82.63 g of Br2(l).Determine the total pressure in the 50.0 L container at equilibrium.

For the reaction;N2(g)+ 3 H2(g)⇌ 2 NH3(g),the equilibrium amount of NH3 will be increased by: I.increasing the pressure II.adding H2 III.removing N2 IV.decreasing the pressure

Consider the following gas phase reaction at 25 °C. N2(g)+ C2H2(g)⇌ 2 HCN(g) 1.600 mol N2(g)and 1.750 mol C2H2(g)are placed in a 1.000 L vessel and the mixture is allowed to react.At equilibrium,there are 1.587 mol N2(g)in the mixture.What is Kc for this reaction at 25 °C?

Write the equilibrium expression Kc for the reaction: Sodium sulfite(aq)+ chloric acid (aq)⇌ sodium chlorate(aq)+ sulfur dioxide(g)+ water(l).

A mixture,containing 0.0750 M HCl(g)and 0.0330 M O2(g)is allowed to come to equilibrium at 480 °C. 4 HCl(g)+ O2(g)⇌ 2 Cl2(g)+ 2 H2O(g) At equilibrium [Cl2] = 0.030 M.What is the value of Kc?

For the following reaction O2(g)⇌ 2 O(g) What conditions favor production of oxygen atoms?

In a reaction at equilibrium involving only gases,a change in pressure of the reaction mixture shifts the position of equilibrium only when:

For the reaction: PCl3(g)+ Cl2(g)⇌ PCl5(g)at 85 °C,Kp = 1.19 If one starts with 2.00 atm pressure of PCl3,1.00 atm pressure of Cl2 and no PCl5,what is the partial pressure of PCl5(g)at equilibrium?

For CO2(g)+ H2(g)⇌ CO(g)+ H2O(g),Kc = [CO][H2]/[CO2][H2],if there are 1.43 mols each of CO and H2O,0.572 mol H2 and 4.572 mols CO2,in a 4.0 L container at equilibrium,what is Kc?

For the reaction below CO(g)+ 2 H2(g)⇌ CH3OH(g) The equilibrium concentrations at 483 K are [CO] = 0.0753 M,[H2] = 0.151 M,and [CH3OH] = 0.0247 M.Calculate the value of Kc.

Changes in temperature cause change in the equilibrium position.

For 2 NO2(g)⇌ N2O4(g),Kc = [N2O4]/[NO2]2.At equilibrium there are 0.0270 mol N2O4 and 0.450 mol NO2 in a 50.0-L container.What is Kc?

Consider the following reaction at a certain temperature. 2 SO3(g)⇌ 2 SO2(g)+ O2(g) When the initial concentration of SO3(g)is 0.128 M,the concentration of oxygen gas at equilibrium is found to be 0.0130 M.Calculate Kc for this reaction.

For the reaction: H2(g)+ I2(g)⇌ 2 HI(g),Kc = 92.0 When equilibrium concentrations of HI and I2 are [HI] = 0.115 M and [I2] = 0.250 M,the equilibrium concentration of [H2] is:

What will happen to the equilibrium in the reaction 2 A(g)⇌ B(g)+ C(g),Kc = 1.25 at 300 K,if a catalyst is added?

For the reaction: CH4(g)+ 2 H2O(g)⇌ CO2(g)+ 4 H2(g),ΔrH° = +190 kJ,when the temperature is raised to 1200 K:

Consider the following equation: N2O4(g)⇌ 2 NO2(g),Kc = 5.8 × 10-3 If the initial concentration of N2O4(g)= 0.040 M and the initial concentration of NO2(g)is 0 M,what is the equilibrium concentration of N2O4(g)?

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Consider the equilibrium system: N₂O₄(g)⇌ 2 NO₂(g)for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute At equilibrium.

For the reaction;N₂(g)+ 3 H₂(g)⇌ 2 NH₃(g),the equilibrium amount of NH₃ will be increased by: I.increasing the pressure II.adding H₂ III.removing N₂ IV.decreasing the pressure

Consider the following gas phase reaction at 25 °C. N₂(g)+ C₂H₂(g)⇌ 2 HCN(g) 1.600 mol N₂(g)and 1.750 mol C₂H₂(g)are placed in a 1.000 L vessel and the mixture is allowed to react.At equilibrium,there are 1.587 mol N₂(g)in the mixture.What is K_c for this reaction at 25 °C?

Write the equilibrium expression K_c for the reaction: Sodium sulfite(aq)+ chloric acid (aq)⇌ sodium chlorate(aq)+ sulfur dioxide(g)+ water(l).

A mixture,containing 0.0750 M HCl(g)and 0.0330 M O₂(g)is allowed to come to equilibrium at 480 °C. 4 HCl(g)+ O₂(g)⇌ 2 Cl₂(g)+ 2 H₂O(g) At equilibrium [Cl₂] = 0.030 M.What is the value of K_c?

For the following reaction O₂(g)⇌ 2 O(g) What conditions favor production of oxygen atoms?

For the reaction: PCl₃(g)+ Cl₂(g)⇌ PCl₅(g)at 85 °C,K_p = 1.19 If one starts with 2.00 atm pressure of PCl₃,1.00 atm pressure of Cl₂ and no PCl₅,what is the partial pressure of PCl₅(g)at equilibrium?

For CO₂(g)+ H₂(g)⇌ CO(g)+ H₂O(g),K_c = [CO][H₂]/[CO₂][H₂],if there are 1.43 mols each of CO and H₂O,0.572 mol H₂ and 4.572 mols CO₂,in a 4.0 L container at equilibrium,what is K_c?

For the reaction below CO(g)+ 2 H₂(g)⇌ CH₃OH(g) The equilibrium concentrations at 483 K are [CO] = 0.0753 M,[H₂] = 0.151 M,and [CH₃OH] = 0.0247 M.Calculate the value of K_c.

For 2 NO₂(g)⇌ N₂O₄(g),K_c = [N₂O₄]/[NO₂]².At equilibrium there are 0.0270 mol N₂O₄ and 0.450 mol NO₂ in a 50.0-L container.What is K_c?

Consider the following reaction at a certain temperature. 2 SO₃(g)⇌ 2 SO₂(g)+ O₂(g) When the initial concentration of SO₃(g)is 0.128 M,the concentration of oxygen gas at equilibrium is found to be 0.0130 M.Calculate K_c for this reaction.

For the reaction: H₂(g)+ I₂(g)⇌ 2 HI(g),K_c = 92.0 When equilibrium concentrations of HI and I₂ are [HI] = 0.115 M and [I₂] = 0.250 M,the equilibrium concentration of [H₂] is:

What will happen to the equilibrium in the reaction 2 A(g)⇌ B(g)+ C(g),K_c = 1.25 at 300 K,if a catalyst is added?

For the reaction: CH₄(g)+ 2 H₂O(g)⇌ CO₂(g)+ 4 H₂(g),Δ_rH° = +190 kJ,when the temperature is raised to 1200 K:

Consider the following equation: N₂O₄(g)⇌ 2 NO₂(g),K_c = 5.8 × 10^-3 If the initial concentration of N₂O₄(g)= 0.040 M and the initial concentration of NO₂(g)is 0 M,what is the equilibrium concentration of N₂O₄(g)?