Hydrogen gas and carbon dioxide gas are present in equal molar quantities at $800\,\text{K}$. A reversible reaction occurs. $\text{H}_2(g) + \text{CO}_2(g) \rightleftharpoons \text{H}_2\text{O}(g) + \text{CO}(g)$ When equilibrium is reached, the partial pressures of $\text{H}_2$ and $\text{CO}_2$ are each $10.0\,\text{kPa}$. At $800\,\text{K}$, $K_p$ is $0.288$. Calculate the partial pressure of $\text{CO}$ in the equilibrium mixture.
- A$5.37\,\text{kPa}$
- B$18.6\,\text{kPa}$
- C$28.8\,\text{kPa}$
- D$347\,\text{kPa}$