Question:medium
The reaction between N$_2$ and O$_2$ is carried out in a sealed vessel at $300,K$. At equilibrium, $[N_2]=2\times10^{-3}M$, $[O_2]=4\times10^{-3}M$ and $[NO]=2\times10^{-3}M$. What is the value of $K_p$ for the reaction $N_2(g)+O_2(g)\rightleftharpoons2NO(g)$ at $300,K$? $(R=0.08,bar,lit,mol^{-1}K^{-1})$
The reaction between N$_2$ and O$_2$ is carried out in a sealed vessel at $300,K$. At equilibrium, $[N_2]=2\times10^{-3}M$, $[O_2]=4\times10^{-3}M$ and $[NO]=2\times10^{-3}M$. What is the value of $K_p$ for the reaction $N_2(g)+O_2(g)\rightleftharpoons2NO(g)$ at $300,K$? $(R=0.08,bar,lit,mol^{-1}K^{-1})$
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Chemistry Tip: When $\Delta n=0$, always remember $K_p = K_c$.
Updated On: Apr 27, 2026
- $0.5$
- $12$
- $120$
- $5$
- $50$
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The Correct Option is B
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