Question

At 600 K, 2 mol of NO are mixed with 1 mol of $O_2$.

$\begin{array}{l}2NO\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO_2\left(g\right)\end{array}$

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)

Answer 1

The correct answer is : 2
2NO+ O2 → 2NO
2 1 -
2-2x 1-x 2x
1.2 0.6 0.8
$K_p=\frac{(\frac{0.8}{2.6})^2}{(\frac{1.2}{2.6})^2(\frac{0.6}{2.6})}$
$=1.925 ≈2$