Nitrogen monoxide and oxygen undergo a reversible reaction described by the equation below. $2\text{NO}(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}_2(g)$ The partial pressures of the substances in an equilibrium mixture are listed here: $P_{\text{NO}} = 10\,\text{kPa}$, $P_{\text{O}_2} = 30\,\text{kPa}$, $P_{\text{NO}_2} = 20\,\text{kPa}$ What is the numerical value of the equilibrium constant, $K_p$, for this equilibrium?
- A$6.67 \times 10^{-2}$
- B$1.33 \times 10^{-1}$
- C$7.50$
- D$15.0$