The value of ΔH° for the reaction 3 O2(g) ⇌ 2 O3(g) is +285 kJ. Does the equilibrium constant for this reaction increase or decrease when the temperature increases? Justify your answer using Le Châtelier’s principle.

Verified step by step guidance

1. Step 1: Understand the reaction and the given information. The reaction is 3 O2(g) ⇌ 2 O3(g) with a ΔH° of +285 kJ, indicating that the reaction is endothermic (absorbs heat).
2. Step 2: Recall Le Châtelier’s principle, which states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the system will adjust to counteract the change and restore a new equilibrium.
3. Step 3: Consider the effect of temperature on an endothermic reaction. For an endothermic reaction, increasing the temperature adds heat to the system, which can be considered as a reactant.
4. Step 4: Apply Le Châtelier’s principle. Since the reaction is endothermic, increasing the temperature will shift the equilibrium to the right, favoring the formation of products (O3) to absorb the added heat.
5. Step 5: Relate the shift in equilibrium to the equilibrium constant (K). As the equilibrium shifts to the right, the concentration of products increases relative to reactants, leading to an increase in the equilibrium constant (K) with an increase in temperature.