Question

# The equilibrium constant for the reaction $$\mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})=2\mathrm{N}\mathrm{O}(\mathrm{g})$$at temperature $$\mathrm{T}$$ is $$4\times 10^{-4}$$. The value of $$\mathrm{K}_{\mathrm{c}}$$ for the reaction:$$NO(g)$$ $$=\displaystyle \frac{1}{2}\mathrm{N}_{2}(\mathrm{g})+\frac{1}{2}\mathrm{O}_{2}(\mathrm{g})$$ at the same temperature is :

A
2.5×102
B
50
C
4×104
D
0.02

Solution

## The correct option is A $$50$$The equilibrium constant for the reaction $$\mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})= 2\mathrm{N}\mathrm{O}(\mathrm{g})$$at temperature $$\mathrm{T}$$ is $$4\times 10^{-4}$$. The value of $$\mathrm{K}_{\mathrm{c}}$$ for the reaction:NO(g) $$=\displaystyle \frac{1}{2}\mathrm{N}_{2}(\mathrm{g})+\frac{1}{2}\mathrm{O}_{2}(\mathrm{g})$$ at the same temperature is $$\displaystyle \frac {1}{\sqrt {K_c}} = \frac {1}{\sqrt {4 \times 10^{-4}}} = 50$$Note: The second reaction is obtained when the first reaction is reversed and divided by 2.Chemistry

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