Question

At 1000 K, the equilibrium constant for the reaction:

2NO (g) + Br₂ (g)↔2NOBr (g) is Kp = 0.013.

Calculate Kp for the reverse reaction:
2NOBr ↔ 2NO (g) + Br₂ (g)

a. 0.013
b. 1.6 x 10⁻⁴
c. 77
d. 0.99

Answer 1

The equilibrium constant for the reverse reaction 2NOBr ↔ 2NO (g) + Br₂ (g) can be found by taking the inverse of the equilibrium constant for the forward reaction. At 1000 K, Kp for the reverse reaction is approximately 77.

Step-by-step explanation:

To calculate the equilibrium constant (Kp) for the reverse reaction 2NOBr ↔ 2NO (g) + Br₂ (g) when given the equilibrium constant for the forward reaction (2NO (g) + Br₂ (g) ↔ 2NOBr (g)) which is Kp = 0.013 at 1000 K, use the relationship Kp(reverse) = 1 / Kp(forward). So the Kp for the reverse reaction is Kp(reverse) = 1 / 0.013.

After computing the inverse of the given Kp value:

Kp(reverse) = 1 / 0.013 ≈ 76.9, or as scientifically notated, approximately 7.7 × 10².

Hence, the correct answer for Kp of the reverse reaction at 1000 K is c. 77.