The reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) is exothermic, ΔHº_rxn=-210 kJ/mol. Which one of the following is correct?

Question

Quizplus · Accepted Answer

The reaction is exothermic, meaning that increasing the temperature will shift the equilibrium towards the reactants side, resulting in a decrease in K_P. Therefore, K_P at 1200 K is smaller than K_P at 800 K. Pressure does not affect the equilibrium constant for a reaction, so C and E are incorrect. Option A is incorrect since increasing the temperature decreases K_P. Option B is also incorrect since temperature does affect the equilibrium constant.

The Reaction 2H2O2(g) 2H2O(g) + O2(g) Is Exothermic, ΔHºrxn

The Reaction 2H₂O₂(g) 2H₂O(g) + O₂(g) Is Exothermic, ΔHº_rxn