At 600K, 2 mol of NO are mixed with 1 mol of O₂.

2NO_(g) + O₂(g) $⇄$ 2NO₂(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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Vishal Baghel | Contributor-Level 10

7 months ago

$2 N O_{(g)} + O_{2 (g)} ? 2 N O_{2} (g)$

Initial moles2mol1 mol

At equilibrium (2 – 2x) mole (1 – x) mol2x mol

$n o_{2} \Rightarrow (1 - x) = 0.6$

$∴ x = 0.4$

$n_{N O} = 2 - 2 x = 2 - 2 * 0.4$

= 2 0.8 = 1.2

$n_{N O_{2}} = 2 x = 2 * 0.4 = 0.8$

$∴ K p = \frac{{(\frac{0.8}{2.6})}^{2}}{{(\frac{1.2}{2.6})}^{2} (\frac{0.6}{2.6})}$

= 1.925

the nearest integer = 2.

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