Cyclobutane gas decomposes to butene gas when heated.

The equilibrium constant K_c for this reaction is 3.0×10⁴ at 700 K. What is the value of K_p at 700 K?

Calculate K_c for each reaction. b. CH₄(g) + H₂O(g) ⇌ CO(g) + 3 H₂(g), K_p = 2.5 x 10³ (at 1200 K)

At 298 K, the K_c for the reaction 2 H₂S(g) ⇋ 2 H₂(g) + S₂(g) is 1.67×10⁻⁷. What is the K_c for the reaction H₂S(g) ⇋ H₂(g) + 1/2 S₂(g) at the same temperature?

The reaction 2 SO₃(g) + N₂(g) ⇌ 2 NO₃(g) + S₂(g) has K_p of 4.5 x 10^-7 at 1000 K. What is the K_p of the reaction below at the same temperature?

2 NO₃(g) + S₂(g) ⇌ 2 SO₃(g) + N₂(g)

Consider the following equilibrium reaction: 2 NOBr(g) + Cl₂(g) ⇌ 2 NO(g) + 2 BrCl(g), ΔH° = +47.4 kJ. 

(a) How will the concentration of NO change when the temperature of the system is lowered?

(b) How will the equilibrium constant (K_c) change when the temperature of the system is increased?

Explain your answer using Le Chatelier's principle.

The reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) has the following values at 298 K: K_p = 6.2×10⁵  and ΔH° = –92.2 kJ. Consider the following changes below which will result in an increase in the partial pressure of NH₃ at equilibrium. Which of the changes will result in the highest increase in the partial pressure of NH₃? Justify your answer. 

I. Adding 0.20 mol of N₂

III. Adding 0.20 mol of H₂

III. Lowering the temperature to 250 K

A. Adding 0.20 mol of N₂ will result in the highest increase in partial pressure of NH₃ because it will produce a greater amount of NH₃.

B. Adding 0.20 mol of H₂ will result in the highest increase in partial pressure of NH₃ because it is the limiting reactant.

C. Lowering the temperature to 250 K will result in the highest increase in partial pressure of NH₃ because it will shift the equilibrium reaction to the right.

D. All of the above will result in the same increase in the partial pressure of NH₃.

Determine the condition that will increase the amount of C₄H₈Br₂ at equilibrium for the endothermic reaction: 

C₄H₈ (g) + Cl₂ (g) ⇌ C₄H₈Br₂ (g)

a. removing Cl₂ from the mixture

b. increasing the volume of the reaction

c. increasing the amount of C₄H₈

d. increasing the temperature of the reaction

A reaction chamber initially contains a mixture of NO(g) and Cl₂(g) at 1069 K, with pressures of 4.564 atm and 2.801 atm, respectively. The following reaction occurs: 2 NO(g) + Cl₂(g) ⇌ 2 NOCl(g). Calculate the value of K_c if the total pressure at equilibrium is 5.45 atm.

Consider the following reaction 375°C: SO₂(g) + Cl₂(g) ⇌ SO₂Cl₂(g), K_c = 25.9. 

In a reaction vessel, 2.50 M of SO₂(g) and 2.25 M of Cl₂(g) were mixed. Calculate the concentration of all species once equilibrium is reached at 375°C.

The reaction of hydrogen (H₂) and iodine (I₂) produces hydrogen iodide (HI) according to the following equation:

H_2(g) + I_2(s) ⇌ 2 HI_(g)

An equilibrium mixture contains the following concentrations/amounts of the reactants and products in a 1.00 L container: H₂ = 0.234 mol, HI = 0.348 mol and I₂ = 10.0 g.

If an additional 0.0700 moles of H₂ are added to the reaction mixture, how many moles of HI are produced when the equilibrium is reestablished?

Consider the following reaction 2 LM ⇌ L₂ + M₂ with an equilibrium constant of K_c = 0.25 The diagram below shows a mixture of the molecules L₂ (yellow), M₂ (black), and LM. Determine the correct statement about the mixture. 

The following reaction has an equilibrium constant of 0.953 at 125 °C. 

N₂H₄ (g) → N₂ (g) + 2 H₂ (g)

At 125 °C, 3.00x10^-3 M N₂H₄, 4.50x10^-5 M N₂, 3.50x10^-5 M H₂ were mixed in a flask. Will the mixture reach equilibrium? If not, in which direction should the reaction proceed to reach equilibrium?

A sealed container with the gases at equilibrium at 298 K contains P_N2O4 = 0.512 atm and P_N2O = 0.0607 atm. A second container, under the same temperature, contains P_N2O4 = 0.163 atm and P_N2O = 0.0342 atm. The gases follow the reaction: N₂O₄(g) ⇌ 2 N₂O(g). Identify if the second reaction is at equilibrium. If it is not in equilibrium, calculate the equilibrium partial pressure of N₂O.