For the equation shown, an equilibrium is reached at a temperature of $700\,\text{K}$. The equilibrium constant, $K_p$, for this reaction is $9.80\,\text{kPa}$. At equilibrium, the partial pressure of $\text{N}_2\text{O}_4$ is $80.0\,\text{kPa}$. $\text{N}_2\text{O}_4\text{(g)} \rightleftharpoons 2\text{NO}_2\text{(g)}$ What is the partial pressure of $\text{NO}_2$ at equilibrium?
- A$8.16\,\text{kPa}$
- B$28.0\,\text{kPa}$
- C$66.6\,\text{kPa}$
- D$784\,\text{kPa}$