Sulfur dioxide and oxygen react to form sulfur trioxide. This reaction can proceed in both directions. $2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)$ $K_p = 2.96 \times 10^{-9}\ \text{Pa}^{-1}$ at $700\,^{\circ}\text{C}$. The mixture is left to reach equilibrium at $700\,^{\circ}\text{C}$. The partial pressure of O$_2$(g) is $375\ \text{kPa}$ and the partial pressure of SO$_3$(g) is $20.3\ \text{kPa}$. What is the partial pressure of SO$_2$(g)?
- A$19.3\ \text{kPa}$
- B$609\ \text{kPa}$
- C$18\ 300\ \text{kPa}$
- D$609\ 000\ \text{kPa}$