Question

${AB}_2$ dissociates as ${AB}_{2\left(g\right)}\rightleftharpoons {AB}_{\left(g\right)}+B_{\left(g\right)}$. When the initial pressure of ${AB}_2$ is 600 mm of Hg, the total equilibrium pressure is 800 mm of Hg. Calculate $K_p$ for the reaction, assuming that the volume of the system remain unchanged?

• A. 50
• B. 100
• C. 166.8
• D. 400

Answer 1

The correct option is B 100

${AB}_{2\left(g\right)}\rightleftharpoons {AB}_{\left(g\right)}+B_{\left(g\right)}$

$600$ $-$ $-$

$600-x$ $x$ $x$

$x=200$

$K_P=\frac{P_{AB}.P_B}{P_{{AB}_2}}=\frac{200\times 200}{400}=100$