Question

The partial pressures of an equilibrium mixture of N₂O₄(g) and NO₂(g) are P_N2O4 = 0.34 atm and P_NO2 = 1.20 atmat a certain temperature. The volume of the container is doubled. Calculate the partial pressures of the two gases when a new equilibrium is established.

Short answer

The new equilibrium partial pressures of N₂O₄(g) and NO₂(g) are 0.12 atm and 0.704 atm, respectively.

Step-by-step solution

Equilibrium constant expression in terms of partial pressure

The balanced chemical equation for the given reaction is written below:

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$

The corresponding equilibrium constant, K_pexpression in terms of partial pressures, is given below:

${\text{K}}_{\text{p}}\text{=}\frac{{{\text{P}}_{ {\text{NO}}_{\text{2}}}}^{\text{2}}}{{\text{P}}_{{\text{N}}_{\text{2}}{\text{O}}_{\text{4}}}}$

The equilibrium partial pressures of N₂O₄(g) and NO₂(g) are 0.34 atm and 1.20 atm, respectively.