Chapter 14, Problem 14.126QP

A container with a volume of 1.500 L was evacuated and then filled at low temperature with 0.0500 mol liquid dinitrogen tetroxide, N₂O₄. As the temperature was raised, this substance formed nitrogen dioxide, NO:

${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}(g)\stackrel{}{\rightleftharpoons }{\text{2NO}}_2(g)$

If the pressure of this reaction mixture at equilibrium at 25.0°C was 0.971 atm, what was the total moles of gas in this mixture? What are the moles of NO₂ and moles of N₂O₄? What are the partial pressures of NO₂ and N₂O₄? What is K_c at 25.0°C?