For 2 N₂O (g) + O₂ (g)→4 NO (g) at 298 K, D H ° = +196 kJ, D G ° = +140 kJ, D S ° = +1.99 J/K. Which of the following changes would always increase the amount of NO at equilibrium?

Question

Quizplus · Accepted Answer

Raising the temperature shifts the equilibrium towards the products in an endothermic reaction (ΔH° = +196 kJ indicates the reaction is endothermic). Lowering the pressure favors the side with more moles of gas; since 3 moles of reactants produce 4 moles of NO, reducing pressure shifts the equilibrium towards more NO.

For 2 N2O (G) + O2 (G)→4 NO (G) at 298

For 2 N₂O (G) + O₂ (G)→4 NO (G) at 298