# The equilibrium ${\mathrm{N}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{NO}}_{\left(\mathrm{g}\right)}$ established in a reaction vessel of 2.5 L capacity.The amount of  taken at the start were respectively 2 moles and 4 moles. Half a mole of nitrogen has been used up at equilibrium. The molar concentration of nitric oxide is

1. A

0.2

2. B

0.4

3. C

0.6

4. D

0.1

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### Solution:

${\mathrm{N}}_{2\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{NO}}_{\left(\mathrm{g}\right)}$

Initial : 2 4 0

Conc. at equilibrium

2-X   4-X  2X

According to question on ½ mole of${\mathrm{N}}_{2}$ is used up at equilibrium,

so $\mathrm{x}=\frac{1}{2}$

${\mathrm{n}}_{0}=2\mathrm{X}=2\left(1/2\right)=1$

Molar concentration

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