Question

One mole of $N_2{O}_4$ is heated in a flask with a volume of $0.1{dm}^3$. At equilibrium, $1.708$ moles of ${NO}_2$ and $0.146$ mole of $N_2{O}_4$ were found ${134}^{o}C$. The equilibrium constant will be:

• A. $250mold{m}^{-3}$
• B. $300mol{dm}^{-3}$
• C. $200mol{dm}^{-3}$
• D. $230mol{dm}^{-3}$

Answer 1

The correct option is C $200mol{dm}^{-3}$

One mole of $N_2{O}_4$ is heated in a flask with a volume of $0.1{dm}^3$. At equilibrium, $1.708$ moles of ${NO}_2$ and $0.146$ mole of $N_2{O}_4$ were found ${134}^{o}C$. The equilibrium constant will be $200mol{dm}^{-3}$.
$N_2{O}_4\rightleftharpoons 2N{O}_2$

$K=\frac{[N{O}_2{]}^2}{\left[N_2{O}_4\right]}$

$K=\frac{(\frac{1.708mol}{0.1d{m}^3}{)}^2}{\frac{0.146mol}{0.1d{m}^3}}$

$K=200mol{dm}^{-3}$.