The decomposition of N2O4  to  NO2 is carried out at 280 K in chloroform. When equilibrium has been established, 0.2 mol of N2O4  and 2 × 10-3  mol of  NO2 are present in 2 litre solution. The equilibrium constant for reaction N2O4  ⇌  2NO2 is

# The decomposition of  is carried out at 280 K in chloroform. When equilibrium has been established, 0.2 mol of  are present in 2 litre solution. The equilibrium constant for reaction  is

1. A

2. B

3. C

4. D

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### Solution:

$\mathrm{K}=\frac{{\left[{\mathrm{NO}}_{2}\right]}^{2}}{\left[{\mathrm{N}}_{2}{\mathrm{O}}_{4}\right]}$ =  = $\frac{{10}^{-6}}{{10}^{-1}}={10}^{-5}$

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