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

What is the value for Kc if [CO] = 0.025, [H2] = 0.013 and [CH3OH] = 0.0028 for the following reaction? CH3OH(g) ⇌ CO(g) + 2 H2(g)

A) 1.5 × 10-3 B) 0.12 C) 6.6 × 102 D) 8.6 E) 9.1 × 10-7 A) 1.5 × 10-3 B) 0.12 C) 6.6 × 102 D) 8.6 E) 9.1 × 10-7

In the reaction: 2 N2O(g) + N2H4(g) ⇌ 3 N2(g) + 2 H2O(g), One starts with 0.10 mol N2O and 0.25 mol N2H4 in a 10.0 L container. If there are 0.06 mol N2O at equilibrium, how many moles of N2 are present?

A) 0.02 B) 0.04 C) 0.06 D) 0.09 E) 0.07 A) 0.02 B) 0.04 C) 0.06 D) 0.09 E) 0.07

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) ⇌ BrCl(g) At the point of equilibrium there were 82.63 g of Br2(l). Compute the value of Kc for this reaction.

A) 0.0699 B) 1.18 C) 0.849 D) 3.50 E) 0.849. A) 0.0699 B) 1.18 C) 0.849 D) 3.50 E) 0.849.

For the reaction: CH4(g) + 2H2O(g) ⇌ CO2(g) + 4H2(g) ΔH° = +190 kJ add H2(g):

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

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ raise the temperature to 1200 K:

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

Consider the following reaction at a certain temperature. 2SO3(g) ⇌ 2SO2(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 x 10-4 B) 1.62 x 10-2 C) 7.64 x 10-5 D) 1.47 x 10-3 A) 8.45 x 10-4 B) 1.62 x 10-2 C) 7.64 x 10-5 D) 1.47 x 10-3

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

Consider the reaction: CH4(g) + 4 Cl2(g) ⇌ CCl4(l) + 4 HCl(g) &emsp; ΔH° -398 kJ/mol The equilibrium is displaced to the right if:

A) the temperature is raised B) the pressure is lowered C) some carbon tetrachloride is removed D) some hydrogen chloride is added E) some chlorine gas is removed A) the temperature is raised B) the pressure is lowered C) some carbon tetrachloride is removed D) some hydrogen chloride is added E) some chlorine gas is removed

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container. What will be the equilibrium value of [N2O]?

A) 0.928 M B) 0.0822 M C) 0.358 M D) 0.379 M E) 0.042 M A) 0.928 M B) 0.0822 M C) 0.358 M D) 0.379 M E) 0.042 M

Exam 15: Principles of Chemical Equilibrium

For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) , Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H₂] = 0.045, [H₂O] = 0.025, and [CH₄] = 0.046M, in which direction will a reaction occur and why?

(Multiple Choice)

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Question 41

Consider the following reaction: POCl₃(g) ⇌ POCl(g) + Cl₂(g) Kc = 0.450 A sample of pure POCl₃(g) was placed in a reaction vessel and allowed to decompose according to the above reaction. At equilibrium, the concentrations of POCl(g) and Cl₂(g) were each 0.150 M. What was the initial concentration of POCl₃(g)?

(Multiple Choice)

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Question 42

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 43

What is the value for Kc if [CO] = 0.025, [H₂] = 0.013 and [CH₃OH] = 0.0028 for the following reaction? CH₃OH(g) ⇌ CO(g) + 2 H₂(g)

(Multiple Choice)

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Question 44

For the reaction PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl₅] = 0.2 M, [PCl₃] = 0.20 M, and [Cl₂] = 2.25 M, in which direction will a reaction occur and why?

(Multiple Choice)

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Question 45

In the reaction: 2 N₂O(g) + N₂H₄(g) ⇌ 3 N₂(g) + 2 H₂O(g), One starts with 0.10 mol N₂O and 0.25 mol N₂H₄ in a 10.0 L container. If there are 0.06 mol N₂O at equilibrium, how many moles of N₂ are present?

(Multiple Choice)

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Question 46

For which of the following reactions does Kp = Kc?

(Multiple Choice)

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Question 47

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) ⇌ BrCl(g) At the point of equilibrium there were 82.63 g of Br₂(l). Compute the value of Kc for this reaction.

(Multiple Choice)

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Question 48

For the reaction: CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) ΔH° = +190 kJ add H₂(g):

(Multiple Choice)

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Question 49

For the reaction: CH₄(g) + 2 H₂O(g) ⇌ CO₂(g) + 4 H₂(g) ΔH° = +190 kJ raise the temperature to 1200 K:

(Multiple Choice)

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Question 50

Consider the following reaction at a certain temperature. 2SO₃(g) ⇌ 2SO₂(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.

(Multiple Choice)

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Question 51

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)?

(Multiple Choice)

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Question 52

Write the equilibrium constant expression for the following reaction: 6 CO₂(g) + 6 H₂O(l) ⇌ C₆H₁₂O₆(s) + 6 O₂(g)

(Multiple Choice)

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Question 53

According to Le Chatelier's Principle:

(Multiple Choice)

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Question 54

Choose the INCORRECT statement.

(Multiple Choice)

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Question 55

What is the equilibrium constant expression for: 4 NH₃(g) + 5 O₂(g) ⇌ 4 NO(g) + 6 H₂O(g)

(Multiple Choice)

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Question 56

Consider the reaction: CH₄(g) + 4 Cl₂(g) ⇌ CCl₄(l) + 4 HCl(g) ΔH° -398 kJ/mol The equilibrium is displaced to the right if:

(Multiple Choice)

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Question 57

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N₂O₄ and 2 moles of NO₂ are introduced into a 5.0 liter container. What will be the equilibrium value of [N₂O]?

(Multiple Choice)

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Question 58

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container, compute PN₂O₄ at equilibrium.

(Multiple Choice)

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Question 59

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 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 PN₂O₄ at equilibrium.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 99

Exam 15: Principles of Chemical Equilibrium

For the reaction CO(g) + 3 H2(g) ⇌ H2O(g) + CH4(g) , Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H2] = 0.045, [H2O] = 0.025, and [CH4] = 0.046M, in which direction will a reaction occur and why?

What is the value for Kc if [CO] = 0.025, [H2] = 0.013 and [CH3OH] = 0.0028 for the following reaction? CH3OH(g) ⇌ CO(g) + 2 H2(g)

For the reaction PCl5 (g) ⇌ PCl3 (g) + Cl2 (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl5] = 0.2 M, [PCl3] = 0.20 M, and [Cl2] = 2.25 M, in which direction will a reaction occur and why?

In the reaction: 2 N2O(g) + N2H4(g) ⇌ 3 N2(g) + 2 H2O(g), One starts with 0.10 mol N2O and 0.25 mol N2H4 in a 10.0 L container. If there are 0.06 mol N2O at equilibrium, how many moles of N2 are present?

For which of the following reactions does Kp = Kc?

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) ⇌ BrCl(g) At the point of equilibrium there were 82.63 g of Br2(l). Compute the value of Kc for this reaction.

For the reaction: CH4(g) + 2H2O(g) ⇌ CO2(g) + 4H2(g) ΔH° = +190 kJ add H2(g):

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ raise the temperature to 1200 K:

Consider the following reaction at a certain temperature. 2SO3(g) ⇌ 2SO2(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.

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)?

Write the equilibrium constant expression for the following reaction: 6 CO2(g) + 6 H2O(l) ⇌ C6H12O6(s) + 6 O2(g)

According to Le Chatelier's Principle:

Choose the INCORRECT statement.

What is the equilibrium constant expression for: 4 NH3(g) + 5 O2(g) ⇌ 4 NO(g) + 6 H2O(g)

Consider the reaction: CH4(g) + 4 Cl2(g) ⇌ CCl4(l) + 4 HCl(g) ΔH° -398 kJ/mol The equilibrium is displaced to the right if:

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5.0 liter container. What will be the equilibrium value of [N2O]?

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container, compute PN2O4 at equilibrium.

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 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 PN2O4 at equilibrium.

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For the reaction CO(g) + 3 H₂(g) ⇌ H₂O(g) + CH₄(g) , Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H₂] = 0.045, [H₂O] = 0.025, and [CH₄] = 0.046M, in which direction will a reaction occur and why?

What is the value for Kc if [CO] = 0.025, [H₂] = 0.013 and [CH₃OH] = 0.0028 for the following reaction? CH₃OH(g) ⇌ CO(g) + 2 H₂(g)

For the reaction PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g) Kc = 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PCl₅] = 0.2 M, [PCl₃] = 0.20 M, and [Cl₂] = 2.25 M, in which direction will a reaction occur and why?

In the reaction: 2 N₂O(g) + N₂H₄(g) ⇌ 3 N₂(g) + 2 H₂O(g), One starts with 0.10 mol N₂O and 0.25 mol N₂H₄ in a 10.0 L container. If there are 0.06 mol N₂O at equilibrium, how many moles of N₂ are present?

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) ⇌ BrCl(g) At the point of equilibrium there were 82.63 g of Br₂(l). Compute the value of Kc for this reaction.

For the reaction: CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) ΔH° = +190 kJ add H₂(g):

For the reaction: CH₄(g) + 2 H₂O(g) ⇌ CO₂(g) + 4 H₂(g) ΔH° = +190 kJ raise the temperature to 1200 K:

Consider the following reaction at a certain temperature. 2SO₃(g) ⇌ 2SO₂(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.

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)?

Write the equilibrium constant expression for the following reaction: 6 CO₂(g) + 6 H₂O(l) ⇌ C₆H₁₂O₆(s) + 6 O₂(g)

What is the equilibrium constant expression for: 4 NH₃(g) + 5 O₂(g) ⇌ 4 NO(g) + 6 H₂O(g)

Consider the reaction: CH₄(g) + 4 Cl₂(g) ⇌ CCl₄(l) + 4 HCl(g) ΔH° -398 kJ/mol The equilibrium is displaced to the right if:

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assume that 1 mole of N₂O₄ and 2 moles of NO₂ are introduced into a 5.0 liter container. What will be the equilibrium value of [N₂O]?

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 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 PN₂O₄ at equilibrium.