For the reaction N_{2(g)} + O_{2(g)} rightlef | vedclass

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(A) Given the reaction: $N_{2(g)} + O_{2(g)} ightleftharpoons 2NO_{(g)}$ with $K_{c1} = 4 	imes 10^{-4}$.For the target reaction: $NO_{(g)} ightl

Vedclass · Accepted Answer

$50$

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(A) Given the reaction: $N_{2(g)} + O_{2(g)} ightleftharpoons 2NO_{(g)}$ with $K_{c1} = 4 	imes 10^{-4}$.For the target reaction: $NO_{(g)} ightleftharpoons 1/2 N_{2(g)} + 1/2 O_{2(g)}$.This target reaction is obtained by reversing the first reaction and multiplying the coefficients by $1/2$.If a reaction is reversed,the new equilibrium constant $K'$ is $1/K$.If a reaction is multiplied by a factor $n$,the new equilibrium constant $K''$ is $(K')^n$.Here,$n = 1/2$,so $K_{c2} = (1/K_{c1})^{1/2} = \sqrt{1/K_{c1}}$.$K_{c2} = \sqrt{1 / (4 	imes 10^{-4})} = \sqrt{10^4 / 4} = \sqrt{0.25 	imes 10^4} = 0.5 	imes 10^2 = 50$.

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant $(K_c)$ at temperature $T$ is $4 \times 10^{-4}$. What is the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons 1/2 N_{2(g)} + 1/2 O_{2(g)}$ at the same temperature?

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