For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant at temperature $T$ is $4 \times 10^{-4}$. Find the value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$.
- A$2.5 \times 10^2$
- B$50$
- C$4 \times 10^{-4}$
- D$0.02$
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Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
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Which of the following relations is correct?
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