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
\(K_p=\frac{(\frac{0.8}{2.6})^2}{(\frac{1.2}{2.6})^2(\frac{0.6}{2.6})}\)
\(=1.925 ≈2\)