Question
Consider the following equilibrium at 2773K
$\text{H}_2(\text{g})+\text{Cl}_2(\text{g})\rightleftharpoons2\text{HCl}(\text{g})$
Initially $0.25M H_2$ and $0.25MCl_2$ are introduced into a reaction vessel and the system in allowed to attain equilibrium. At equilibrium the concentrations of $H_2(g)$ and $Cl_2(g)$ became $0.0314M$. Calculate $K_c$ and $K_p$.
$\text{H}_2(\text{g})+\text{Cl}_2(\text{g})\rightleftharpoons2\text{HCl}(\text{g})$
Initially $0.25M H_2$ and $0.25MCl_2$ are introduced into a reaction vessel and the system in allowed to attain equilibrium. At equilibrium the concentrations of $H_2(g)$ and $Cl_2(g)$ became $0.0314M$. Calculate $K_c$ and $K_p$.