The reaction 2NO(g) N₂(g)+ O₂(g)is exothermic, $\Delta$Hº_rxn = -180 kJ/mol.Which one of these statements is true?

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in temperature, the system will shift its equilibrium position in a direction that tends to counteract that change. Since the reaction is exothermic, an increase in temperature will cause the system to shift to the left, resulting in a decrease in the concentration of the products and an increase in the concentration of the reactants. Therefore, the value of K will decrease with increasing temperature, and K_p at 1,000 K will be larger than K_p at 2,000 K.

The Reaction 2NO(g) N2(g)+ O2(g)is Exothermic Δ\DeltaΔ Hºrxn = -180 KJ/mol

The Reaction 2NO(g) N₂(g)+ O₂(g)is Exothermic $\Delta$ Hº_rxn = -180 KJ/mol