Le Chatelier's principle and kinetics in the endothermic water-gas shift reaction

Steps:

• Statement 1: Gas moles equal (2 left, 2 right), so high pressure does not shift equilibrium position per Le Chatelier's principle. False.
• Statement 2: Higher temperature increases kinetic energy and collisions, raising rate constant (Arrhenius equation), so rate of H2 formation increases. True.
• Statement 3: Higher pressure raises partial pressures and concentrations of gaseous reactants, accelerating forward rate. True.
• Statement 4: Endothermic (ΔH > 0), so high temperature favors products to absorb heat, shifting equilibrium right per Le Chatelier's principle. True.

Why D is correct:

• D selects statements 2 and 4, accurately capturing temperature's dual role in boosting rate and shifting endothermic equilibrium right.

Why the others are wrong:

• A includes 1 (false, pressure doesn't shift equilibrium with Δn=0).
• B includes 1 (false, as above).
• C only 1 (false, as above).

Final answer: D