Question 1

2.5 moles H₂O and 100 g of C are placed in a 50-L container. At equilibrium for the reaction C(s) + H₂O(g) ⇌ CO(g) + H₂(g), [H₂] = 0.040 M. Which of the following is true?

Accepted Answer

The answer of 2.5 moles H₂O and 100 g of...

Question 2

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

Accepted Answer

The answer of What is the equilibrium constant expression for:...

Question 3

For the decomposition of SO₃(g), Kc = [SO₂]₂[O₂]/[SO₃]₂, at equilibrium, there are 0.090 mol SO₂, 0.110 mol O₂, 0.100 mol SO₃ in a 25.0-L container. What is the value of Kc?

Accepted Answer

The concentrations are [SO₂] = 0.090/25, [O₂] = 0.110/25, [SO₃] = 0.100/25. Plug these into Kc = ([SO₂]²[O₂])/[SO₃]² to find Kc = 3.6 × 10⁻³.

Question 4

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

Accepted Answer

High temperature favors the dissociation of O2 into O atoms due to increased kinetic energy, and low pressure favors the side with more moles of gas, which is the product side with 2O(g).

Question 5

Consider the following equilibrium reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl₅(g) to PCl₃(g) and Cl₂(g) is ________.

Accepted Answer

The answer of Consider the following equilibrium reaction: PCl₃(g) +...

Question 6

In a reaction at equilibrium involving only gases, a pressure change will shift the reaction only when:

Accepted Answer

A pressure change will shift the reaction only when the number of molecules on one side of the balanced equation is different from the number on the other side. This is because a change in pressure affects the concentrations of the gases, and according to Le Chatelier's principle, the system will adjust to counteract the change in pressure. If the number of gas molecules changes, the reaction will shift to the side with fewer gas molecules to decrease pressure or to the side with more gas molecules to increase pressure if the volume is decreased.

Question 7

0.75 mol of N₂ and 1.20 mol of H₂ are placed in a 3.0 liter container. When the reaction N₂(g) + 3H₂(g) ⇌ 2 NH₃(g) reaches equilibrium, [H₂] = 0.100 M. Which of the following is true?

Accepted Answer

The initial concentration of H2 is 1.20 mol / 3.0 L = 0.400 M. At equilibrium, [H2] = 0.100 M, so 0.300 M of H2 reacted. Since the reaction consumes 3 moles of H2 for every 2 moles of NH3 produced, [NH3] = (2/3) * 0.300 M = 0.200 M.

Question 8

Consider the following chemical reaction at equilibrium: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g) This equilibrium can be shifted to the right by:

Accepted Answer

Increasing the volume of the mixture will shift the equilibrium to the side with more moles of gas, which is the right side (4 HCl + 1 O2 = 5 moles) compared to the left side (2 Cl2 + 2 H2O = 4 moles).

Question 9

For 2 NO₂(g) ⇌ N₂O₄(g), Kc = [N₂O₄]/[NO₂]₂. At equilibrium there are 0.0270 mol N₂O₄ and 0.450 mol NO₂in a 50.0-L container. What is Kc?

Accepted Answer

Kc = [N₂O₄]/[NO₂]₂ = (0.0270 mol/50.0 L)/(0.450 mol/50.0 L)² = 6.67

Question 10

For the reaction: CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) ΔH° = +190 kJ add N₂(g) at constant volume and:

Accepted Answer

Adding an inert gas at constant volume does not affect the equilibrium position or the enthalpy change of the reaction.

Question 11

Consider the following gas phase reaction at 25°C. N₂(g) + C₂H₂(g) ⇌ 2 HCN(g) 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?

Accepted Answer

The answer of Consider the following gas phase reaction at...

Question 12

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

Accepted Answer

The answer of For CO₂(g) + H₂(g) ⇌ CO(g) +...

Question 13

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)?

Accepted Answer

Using the equation for Kc, we can set up an ICE table: N₂O₄(g) ⇌ 2 NO₂(g) I 0.040 M 0 M C -x +2x E 0.040-x 2x Now we can plug in the values for equilibrium concentrations into the Kc expression and solve for x: Kc = [NO₂]2 / [N₂O₄] 5.8 × 10^-3 = (2x)2 / (0.040-x) Solving for x gives us: x = 3.3 × 10^-2 Thus, the equilibrium concentration of N₂O₄ is: 0.040 - x = 0.040 - 3.3 × 10^-2 = 3.7 × 10^-2, which corresponds to choice C.

Question 14

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?

Accepted Answer

Adding a catalyst can speed up both the forward and reverse reactions equally, so there is no net effect on the equilibrium position or Kc. The only effect is that the reaction reaches equilibrium faster.

Question 15

For the production of NO₂, Kc = [NO₂]₂/[NO]₂[O₂]. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O₂ and 22.0 mol NO₂. The value of Kc is ________.

Accepted Answer

Kc is calculated using the formula: Kc = [NO2]^2 / ([NO]^2 * [O2]). Concentrations are found by dividing moles by volume. Substituting the given values, Kc = (22.0/2.50)^2 / ((3.00/2.50)^2 * (4.00/2.50)) = 33.6.

Question 16

Equilibrium constant K is constant except when one varies the:

Accepted Answer

The equilibrium constant, K, depends on the temperature of the reaction. When the temperature of the reaction changes, the value of K also changes. The other answer choices may affect the position of the equilibrium but do not affect the value of K.

Question 17

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

Accepted Answer

Increasing the pressure favors the formation of fewer gas molecules, thus shifting the equilibrium towards NH₃. Adding H₂ shifts the equilibrium towards the products to counteract the change.

Question 18

Write the equilibrium constant expression for the following reaction: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

Accepted Answer

The answer of Write the equilibrium constant expression for the...

Question 19

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.

Accepted Answer

The equilibrium constant (Kc) for a reaction is calculated using the concentrations of the reactants and products at equilibrium. For the given reaction, the equilibrium constant expression is:Kc = [SO2]^2[O2] / [SO3]^2Substituting the given equilibrium concentrations into the expression, we get:Kc = (0.0130 M)^2 / (0.128 M)^2 = 8.45 x 10^-4Therefore, the correct answer is A) 8.45 x 10^-4.

Question 20

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

Accepted Answer

The equilibrium constant (Kc) for a reaction is calculated using the concentrations of the reactants and products at equilibrium. For the given reaction, the equilibrium constant expression is:Kc = [CH3OH] / ([CO] * [H2]^2)Substituting the given equilibrium concentrations into the expression, we get:Kc = (0.0247 M) / ((0.0753 M) * (0.151 M)^2) = 14.4Therefore, the value of Kc is 14.4.

Quiz 15: Principles of Chemical Equilibrium

2.5 moles H₂O and 100 g of C are placed in a 50-L container. At equilibrium for the reaction C(s) + H₂O(g) ⇌ CO(g) + H₂(g) , [H₂] = 0.040 M. Which of the following is true?

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

For the decomposition of SO₃(g) , Kc = [SO₂]₂[O₂]/[SO₃]₂, at equilibrium, there are 0.090 mol SO₂, 0.110 mol O₂, 0.100 mol SO₃ in a 25.0-L container. What is the value of Kc?

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

Consider the following equilibrium reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl₅(g) to PCl₃(g) and Cl₂(g) is ________.

In a reaction at equilibrium involving only gases, a pressure change will shift the reaction only when:

0.75 mol of N₂ and 1.20 mol of H₂ are placed in a 3.0 liter container. When the reaction N₂(g) + 3H₂(g) ⇌ 2 NH₃(g) reaches equilibrium, [H₂] = 0.100 M. Which of the following is true?

Consider the following chemical reaction at equilibrium: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g) This equilibrium can be shifted to the right by:

For 2 NO₂(g) ⇌ N₂O₄(g) , Kc = [N₂O₄]/[NO₂]₂. At equilibrium there are 0.0270 mol N₂O₄ and 0.450 mol NO₂in a 50.0-L container. What is Kc?

For the reaction: CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) ΔH° = +190 kJ add N₂(g) at constant volume and:

Consider the following gas phase reaction at 25°C. N₂(g) + C₂H₂(g) ⇌ 2 HCN(g) 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?

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

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) ?

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 production of NO₂, Kc = [NO₂]₂/[NO]₂[O₂]. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O₂ and 22.0 mol NO₂. The value of Kc is ________.

Equilibrium constant K is constant except when one varies the:

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

Write the equilibrium constant expression for the following reaction: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

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.

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

Quiz 15: Principles of Chemical Equilibrium

2.5 moles H2O and 100 g of C are placed in a 50-L container. At equilibrium for the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g) , [H2] = 0.040 M. Which of the following is true?

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

For the decomposition of SO3(g) , Kc = [SO2]2[O2]/[SO3]2, at equilibrium, there are 0.090 mol SO2, 0.110 mol O2, 0.100 mol SO3 in a 25.0-L container. What is the value of Kc?

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

Consider the following equilibrium reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl5(g) to PCl3(g) and Cl2(g) is ________.

In a reaction at equilibrium involving only gases, a pressure change will shift the reaction only when:

0.75 mol of N2 and 1.20 mol of H2 are placed in a 3.0 liter container. When the reaction N2(g) + 3H2(g) ⇌ 2 NH3(g) reaches equilibrium, [H2] = 0.100 M. Which of the following is true?

Consider the following chemical reaction at equilibrium: 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g) This equilibrium can be shifted to the right by:

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?

For the reaction: CH4(g) + 2H2O(g) ⇌ CO2(g) + 4H2(g) ΔH° = +190 kJ add N2(g) at constant volume and:

Consider the following gas phase reaction at 25°C. N2(g) + C2H2(g) ⇌ 2 HCN(g) 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?

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

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) ?

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 production of NO2, Kc = [NO2]2/[NO]2[O2]. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O2 and 22.0 mol NO2. The value of Kc is ________.

Equilibrium constant K is constant except when one varies the:

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

Write the equilibrium constant expression for the following reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g)

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.

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

2.5 moles H₂O and 100 g of C are placed in a 50-L container. At equilibrium for the reaction C(s) + H₂O(g) ⇌ CO(g) + H₂(g) , [H₂] = 0.040 M. Which of the following is true?

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

For the decomposition of SO₃(g) , Kc = [SO₂]₂[O₂]/[SO₃]₂, at equilibrium, there are 0.090 mol SO₂, 0.110 mol O₂, 0.100 mol SO₃ in a 25.0-L container. What is the value of Kc?

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

Consider the following equilibrium reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl₅(g) to PCl₃(g) and Cl₂(g) is ________.

0.75 mol of N₂ and 1.20 mol of H₂ are placed in a 3.0 liter container. When the reaction N₂(g) + 3H₂(g) ⇌ 2 NH₃(g) reaches equilibrium, [H₂] = 0.100 M. Which of the following is true?

Consider the following chemical reaction at equilibrium: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g) This equilibrium can be shifted to the right by:

For 2 NO₂(g) ⇌ N₂O₄(g) , Kc = [N₂O₄]/[NO₂]₂. At equilibrium there are 0.0270 mol N₂O₄ and 0.450 mol NO₂in a 50.0-L container. What is Kc?

For the reaction: CH₄(g) + 2H₂O(g) ⇌ CO₂(g) + 4H₂(g) ΔH° = +190 kJ add N₂(g) at constant volume and:

Consider the following gas phase reaction at 25°C. N₂(g) + C₂H₂(g) ⇌ 2 HCN(g) 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?

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

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) ?

For the production of NO₂, Kc = [NO₂]₂/[NO]₂[O₂]. At equilibrium in a 2.50 L container, there are 3.00 mol NO, 4.00 mol O₂ and 22.0 mol NO₂. The value of Kc is ________.

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

Write the equilibrium constant expression for the following reaction: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g)

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.

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