Consider the following equilibrium:

O2 (g) + 2F2 (g) ↔ 2OF2 (g); Kp = 2.3*10-15

Which of the following statements is true?

a. If the reaction mixture initially contains only OF2 (g), then at equilibrium, the reaction mixture will consist of essentially only O2 (g) and F2 (g).

b. For this equilibrium, Kc=Kp.

c. If the reaction mixture initially contains only OF2 (g), then the total pressure at equilibrium will be less than the total initial pressure.

d. If the reaciton mixture initially contains only O2 (g) and F2 (g), then at equilibrium, the reaction mixture will consist of essentially only OF2 (g).

e. If the reaction mixture initially contains only O2 (g) and F2 (g), then the total pressure at equilibrium will be greater than the total initail pressure.

Question

Chemistry

Guest

31 January, 20:13

Consider the following equilibrium:

O2 (g) + 2F2 (g) ↔ 2OF2 (g); Kp = 2.3*10-15

Which of the following statements is true?

a. If the reaction mixture initially contains only OF2 (g), then at equilibrium, the reaction mixture will consist of essentially only O2 (g) and F2 (g).

b. For this equilibrium, Kc=Kp.

c. If the reaction mixture initially contains only OF2 (g), then the total pressure at equilibrium will be less than the total initial pressure.

d. If the reaciton mixture initially contains only O2 (g) and F2 (g), then at equilibrium, the reaction mixture will consist of essentially only OF2 (g).

e. If the reaction mixture initially contains only O2 (g) and F2 (g), then the total pressure at equilibrium will be greater than the total initail pressure.

+5

Answers (1)

Know the Answer?

Skeeter · Answer 1

a. If the reaction mixture initially contains only OF2 (g), then at equilibrium, the reaction mixture will consist of essentially only O2 (g) and F2 (g).

Explanation:

The answer is a) because the value for Kp is really close to zero (having x10⁻¹⁵), this means that at equilibrium O₂ and F₂ will be significantly more present than OF₂.