Question

$K_p$ for the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2{NH}_3\left(g\right)$, at $298K$ is $5.2\times {10}^{-5}$. What is the value of $K_c$ at $298K$, for the reaction $\frac{1}{2}{N}_2\left(g\right)+\frac{3}{2}{H}_2\left(g\right)\rightleftharpoons {NH}_3\left(g\right)$?

Answer 1

$K_p^{\prime }$ for the reaction $\frac{1}{2}{N}_2\left(g\right)+\frac{3}{2}{H}_2\left(g\right)\rightleftharpoons {NH}_3\left(g\right)$ is $\sqrt{K_p}$ i.s., $\sqrt{5.2\times {10}^{-5}}$

$K_c$ for the reaction $\frac{1}{2}{N}_2\left(g\right)+\frac{3}{2}{H}_2\left(g\right)\rightleftharpoons {NH}_3\left(g\right)$, will be $\left(K_p^{\prime }\right)\times (RT{)}^{\Delta n}$

$=\left[\sqrt{5.2\times {10}^{-5}}\right]\times 0.0821\times 298=1.71\times {10}^{-2}{M}^{-1}$

Here, R is constant.