The equations represent four reversible reactions. For which reaction would the position of equilibrium shift to the right when both the pressure and the temperature are increased?
- A$\text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g)$ (exothermic)
- B$4\text{NO}(g) + 6\text{H}_2\text{O}(g) \rightleftharpoons 4\text{NH}_3(g) + 5\text{O}_2(g)$ (endothermic)
- C$\text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g)$ (endothermic)
- D$2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)$ (exothermic)