Chapter 15.5, Problem 1RC

The following equilibrium constants are given at 500 K:

$\begin{array}{ll}{\text{H}}_{\text{2}}{\text{(g) + Br}}_{\text{2}}\text{(g) }\rightleftarrows \text{ 2 HBr(g)}\hfill & K_p\text{ = 7}{\text{.9 × 10}}^{\text{11}}\hfill \\ {\text{H}}_{\text{2}}\text{(g) }\rightleftarrows \text{ 2 H(g)}\hfill & K_p\text{ = 4}{\text{.8 × 10}}^{-\text{41}}\hfill \\ {\text{Br}}_{\text{2}}\text{(g) }\rightleftarrows \text{ 2 Br}\hfill & K_p\text{ = 2}{\text{.2 × 10}}^{-\text{15}}\hfill \end{array}$

What is the value of K_p for the reaction H + Br ⇄ HBr?

1. (a) K_p = 8.3 × 10⁻⁴⁴
2. (b) K_p = 7.5 × 10⁶⁶
3. (c) K_p = 2.7 × 10³³