Chapter 5, Problem 5.54E

For the reaction

${\text{3O}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{2O}}_{\text{3}}\left(\text{g}\right)$

The equilibrium constant at $1600\text{K}$ is $0.235$. (a) If initially, $1.00\text{atm}$ of ${\text{O}}_{\text{2}}$ were introduced into a chamber at $1600\text{K}$, what are the partial pressures present at equilibrium? (Hint: you will have to solve a cubic equation. There are cubic equation solvers available on the internet.) (b) In a second experiment, $1.00\text{atm}$ of ${\text{O}}_{\text{2}}$ is introduced in a chamber at $1600\text{K}$, along with $0.50\text{atm}$ of $\text{Kr}$. Now, what are the partial pressures present at equilibrium?