Question

For the reaction at equilibrium, 2SO3 ⇌ 2SO2 + O2, ΔH°rxn = 198 kJ/mol. Increasing the reaction temperature would:

a) Shift the equilibrium to the right and decrease the value of the equilibrium constant K.
b) Shift the equilibrium to the left and decrease the value of the equilibrium constant K.
c) Shift the equilibrium to the right and increase the value of the equilibrium constant K.
d) Shift the equilibrium to the left and increase the value of the equilibrium constant K.

Answer 1

Increasing the temperature for the endothermic reaction 2SO3 ⇌ 2SO2 + O2 will shift the equilibrium to the right and increase the value of the equilibrium constant K.

Step-by-step explanation:

For the reaction 2SO3 ⇌ 2SO2 + O2 with ΔH°rxn = 198 kJ/mol, it is crucial to understand how an increase in temperature affects the equilibrium position and the value of the equilibrium constant (K). Since ΔH°rxn is positive, this reaction is endothermic. Applying Le Chatelier's principle, an increase in temperature adds heat to the system, which would shift the equilibrium to favor the endothermic process—thus, the equilibrium will shift to the right, towards the formation of more products (2SO2 and O2). Additionally, as a direct consequence of this shift, the value of the equilibrium constant K will also increase.

In summary, increasing the reaction temperature will:

• Shift the equilibrium to the right (favoring the formation of SO2 and O2).
• Increase the value of the equilibrium constant K.