1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 leftharpoons 2NO2 is

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. The decomposition of $N_{2}O_{4}$ to $NO_{2}$ is carried out at $280$ K in chloroform. When equilibrium has been established, $0.2\, mol$ of $N_{2}O_{4}$ and $2 \times 10^{-3}\, mol$ of $NO_{2}$ are present in $2\, litre$ solution. The equilibrium constant for reaction $N_{2}O_{4} \rightleftharpoons 2NO_{2}$ is

Equilibrium

Solution:

$K=\frac{\left[NO_{2}\right]^{2}}{\left[N_{2}O_{4}\right]}=\frac{\left[2\times\frac{10^{-3}}{2}\right]^{^2}}{\left[\frac{2}{2}\right]}=\frac{10^{-6}}{10^{-1}}=10^{-5}$