At equilibrium, ________.

Which one of the following will change the value of an equilibrium constant?

The equilibrium expression for Kp for the reaction below is ________.

2O₃ (g) ↔ 3O₂ (g)

The Keq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C.

2Cl₂ (g) + 2H₂O (g) ↔ 4HCl (g) + O₂ (g)

What is the value of Keq at this temperature for the following reaction?

2HCl (g) + ½O₂ (g) ↔ Cl₂ (g) + H₂O (g)

The Keq for the equilibrium below is 0.112 at 700.0 °C.

SO₂ (g) + ½O₂ (g) ↔ SO₃ (g)

What is the value of Keq at this temperature for the following reaction?

SO₃ (g) ↔ SO₂ (g) + ½O₂ (g)

Given the following reaction at equilibrium, if Kc = 1.90 × 10¹⁹ at 25.0 °C, Kp = ________.

H₂ (g) + Br₂ (g) ↔ 2 HBr (g)

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?

CO₂ (s) + H₂O (l)↔ H⁺ (aq) + HCO₃^- (aq)

The expression for Kp for the reaction below is ________.

4CuO (s) + CH₄ (g) ↔ CO₂ (g) + 4Cu (s) + 2H₂O (g)

The equilibrium constant for the gas phase reaction

N₂ (g) + 3H₂ (g) ↔ 2NH₃ (g)

is Keq = 4.34 × 10^-3 at 300 °C. At equilibrium, ________.

The equilibrium constant for the gas phase reaction

2NH₃ (g) ↔ N₂ (g) + 3H₂ (g)

is Keq = 230 at 300 °C. At equilibrium, ________.

Of the following equilibria, only ________ will shift to the left in response to a decrease in volume.

In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle?

Consider the following reaction at equilibrium:

2CO₂ (g) ↔ 2CO (g) + O₂ (g) ΔH° = -514 kJ

Le Châtelier's principle predicts that an increase in temperature will ________.

Consider the following reaction at equilibrium.

2CO₂ (g) ↔ 2CO (g) + O₂ (g) ΔH° = -514 kJ

Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.

A sealed 1.0 L flask is charged with 0.500 mol of I₂ and 0.500 mol of Br₂. An equilibrium reaction proceeds:

I₂ (g) + Br₂ (g) ↔ 2IBr (g)

When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is ________.

Given the following reaction:

CO (g) + 2 H₂(g) ↔ CH₃OH (g)

In an experiment, 0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.29 mol of CO remaining. Keq at the temperature of the experiment is ______.

Dinitrogentetraoxide partially decomposes according to the following equilibrium:

N₂O₄ (g) ↔ 2 NO₂ (g)

A 1.00-L flask is charged with 0.0400 mol of N₂O₄. At equilibrium at 373 K, 0.0055 mol of N₂O4 remains. Keq for this reaction is ________.

The equilibrium constant (Kp) for the interconversion of PCl₅ and PCl₃ is 0.0121:

PCl₅ (g) ↔ PCl₃ (g) + Cl₂ (g)

A vessel is charged with PCl₅ giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl₃ is ________ atm.

At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 10³.

2NO (g) ↔ N₂ (g) + O₂ (g)

A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂ is ________ atm.

Given the following reaction at equilibrium, if Kc =5.84 x 10⁵ at 230.0 °C, Kp = ________.

2NO (g) + O₂ (g) ↔ 2NO₂ (g)

Given the following reaction at equilibrium at 450.0 °C:

CaCO₃ (s) ↔ CaO (s) + CO₂ (g)

If P_CO2 = 0.0155 atm, Kc = ________.

Given the following reaction at equilibrium at 300.0 K:

NH₄HS (s) ↔ NH₃ (g) + H₂S (g)

If P_NH3 = P_H2S = 0.105 atm, Kp = ________.

The value of Keq for the following reaction is 0.25:

SO₂ (g) + NO₂ (g) ↔ SO₃ (g) + NO (g)

The value of Keq at the same temperature for the reaction below is ________.

3SO₂ (g) + 3NO₂ (g) ↔ 3SO₃ (g) + 3NO (g)

The Keq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C.

2Cl₂ (g) + 2H₂O (g) ↔ 4HCl (g) + O₂ (g)

What is the value of Keq at this temperature for the following reaction?

8HCl (g) +2O₂ (g) ↔ 4Cl₂ (g) + 4H₂O (g)

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction:

PCl₃ (g) + Cl₂ (g) → PCl₅ (g)

An equilibrium mixture at 450 K contains

P_PCl3=0.224 atm,

P_Cl2 = 0.284 atm, and

P_PCl5 = 4.24 atm. What is the value of Kp at this temperature?

Consider the following chemical reaction:

H₂ (g) + I₂ (g) ↔ 2HI (g)

At equilibrium in a particular experiment, the concentrations of H₂, I₂, and HI were 0.20 M, 0.034 M and 0.55 M respectively. The value of Keq for this reaction is _________.

Dinitrogen tetroxide partially decomposes according to the following equilibrium:

N₂O₄ (g) ↔ 2NO₂ (g)

A 1.000-L flask is charged with 9.20 x 10^-3 mol of N₂O₄. At equilibrium, 5.98 x 10^-3 mol of N₂O₄ remains. Keq for this reaction is ________.

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345.

2SO₂ + O₂ (g) → 2SO₃ (g)

At equilibrium, the partial pressure of SO₂ is 36.9 atm and that of O₂ is 16.8 atm. The partial pressure of SO₃ is ________ atm.

The reaction below is exothermic:

2SO₂ (g) + O₂ (g) ↔ 2SO₃ (g)

Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of SO₃ (g) in the reaction container.

For the endothermic reaction

CaCO₃ (s) ↔ CaO (s) + CO₂ (g)

Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of CO₂.

Consider the following reaction at equilibrium:

2NH₃ (g) ↔ N₂ (g) + 3H₂ (g) ΔH° = +92.4 kJ

Le Châtelier's principle predicts that removing N₂ from the system at equilibrium will result in ________.

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide:

H₂ (g) + Br₂ (g) ↔ 2HBr (g)

A mixture of 0.682 mol of H₂ and 0.440 mol of Br₂ is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.546 mol of H₂ present. At equilibrium, there are ________ mol of Br₂ present in the reaction vessel.

At 24°C, Kp = 0.080 for the equilibrium:

NH₄HS (s) ↔ NH₃ (g) + H₂S (g)

A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH₄HS remains.

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction:

CO (g) + H₂O (g) ↔ CO₂ (g) + H₂ (g)

In an experiment, 0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.22 mol of CO remaining. Keq at the temperature of the experiment is ________.

Nitrosyl bromide decomposes according to the following equation.

2NOBr (g) ↔ 2NO (g) + Br₂ (g)

A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br₂. At equilibrium the flask contained 0.16 mol of NOBr. How many moles of NO and Br₂, respectively, are in the flask at equilibrium?