A mixture of sulfur dioxide and oxygen is in dynamic equilibrium in a closed container of fixed volume at 700 K in the presence of a catalyst:
2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ mol−1 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \quad \Delta H = -197\text{ kJ mol}^{-1} 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ mol−1If the catalyst is completely removed from the container while maintaining a constant temperature and volume, which statement is correct?
The equilibrium constant KcK_cKc increases because the rate of the reverse endothermic reaction is reduced.
The activation energy for the forward reaction increases by 197 kJ mol−1197\text{ kJ mol}^{-1}197 kJ mol−1 more than that for the reverse reaction.
The concentrations of all three gases at equilibrium remain unchanged, but the time required to re-attain equilibrium after a temperature change would increase.
The yield of SO3\text{SO}_3SO3 decreases because the forward reaction is slowed down more than the reverse reaction.
