For the reaction $2AB_{(g)} \rightleftharpoons 2A_{(g)} + B_{2(g)}$,$AB$ dissociates. If the initial pressure of $AB$ is $500 \, mm$ and the total pressure at equilibrium is $625 \, mm$,calculate $K_p$ for the reaction. Assume constant volume.

At $T(K)$,when $1 \ mol$ of $X$ and $1 \ mol$ of $Y$ are heated in a $1 \ L$ flask,$0.5 \ mol$ of $Z$ is formed at equilibrium. The $K_c$ value for the reaction $X_{(g)} + Y_{(g)} \rightleftharpoons Z_{(g)} + A_{(g)}$ is:

For the following reaction in gaseous phase $CO + 1/2 O_2 \to CO_2$,the ratio $K_p/K_c$ is:

$2 \ mol$ $PCl_5$ is heated in a $4 \ L$ closed vessel at a definite temperature. At equilibrium,$55\%$ of $PCl_5$ remains undissociated. Find $K_c$. Reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$

The reaction $A(g) \rightleftharpoons B(g) + C(g)$ was initiated with the amount $a$ of $A(g)$. At equilibrium, it is found that the amount of $A(g)$ remaining is $(a-x)$ at a total pressure of $p$. The equilibrium constant $K_{p}$ of the reaction can be calculated from the expression:

For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,at equilibrium,$P_{CO_2} = 2$ and $P_{CO} = 4$. The value of $K_p$ is: