Question

$k_c$ for the reaction $N_2{O}_4\left(g\right)\leftrightharpoons 2N{O}_2$ is $4.63\times {10}^{-3}$ at ${25}^{o}C$
a. what is the value of $K_p$ at this temperature.
b. At ${25}^{o}C$, if the partial pressure of $N_2{O}_4$(g) at equilibrium is 0.2 atm, calculate equilibrium pressure of $N{O}_2\left(g\right)$.

Answer 1

$N_2{O}_4\rightleftharpoons 2{NO}_2△n=2-1=1$

$K_C=4.63\times {10}^{-3}T={25}^{0}C=298K$

$\left(a\right)$

$K_P=K_C{\left(RT\right)}^{△n}$

$=K_{C}RT=4.63\times {10}^{-3}\times 8.3\times 298$

$=11,451.8\times {10}^{-3}$

$=11.5$