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$At 600 K, 2 mol of NO are mixed with 1 mol of O_{2} . 2 {NO}_{(g)} + O_{2} (g) \overset{}{⇄} 2 {NO}_{2} (g)$
The reaction occurring as above comes to equilibrium under a total pressure of 1 atm. Analysis of the system shows that 0.6 mol of oxygen are present at equilibrium. The equilibrium constant for the reaction is ______. (Nearest integer)

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answer is 2.

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Detailed Solution

$\begin{matrix} 2 N O & + O_{2} \to & 2 N O \\ 2 & 1 & - \\ 2 - 2 X & 1 - x & 2 x \\ 1.2 & 0.6 & 0.8 \end{matrix} K_{p} = \frac{{(\frac{0.8}{2.6})}^{2}}{{(\frac{1.2}{2.6})}^{2} (\frac{0.6}{2.6})} = 1.925$

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