(c) In each case, indicate whether K should increase or decrease with increasing temperature. (i) 2 Mg(s) + O₂ (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I₂(g) (iii) Na₂(g) ⇌ 2 Na(g) (iv) 2 V₂O₅(s) ⇌ 4 V(s) + 5 O₂(g)

검증된 단계별 안내

Identify the type of reaction for each case: exothermic or endothermic. This can often be inferred from the reaction equation or given data.

Apply Le Chatelier's Principle: For an exothermic reaction, increasing temperature shifts the equilibrium to the left, decreasing K. For an endothermic reaction, increasing temperature shifts the equilibrium to the right, increasing K.

For reaction (i) 2 Mg(s) + O2(g) ⇌ 2 MgO(s), determine if the formation of MgO is exothermic or endothermic. Typically, the formation of metal oxides is exothermic.

For reaction (ii) 2 KI(s) ⇌ 2 K(g) + I2(g), consider the phase change from solid to gas, which usually requires energy input, indicating an endothermic process.

For reactions (iii) Na2(g) ⇌ 2 Na(g) and (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g), analyze the stoichiometry and phase changes to determine the enthalpy change, and apply Le Chatelier's Principle accordingly.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how the equilibrium constant (K) will respond to changes in temperature, pressure, or concentration. For example, if a reaction is exothermic, increasing the temperature will shift the equilibrium to favor the reactants, thus decreasing K.

Endothermic and Exothermic Reactions

Reactions can be classified as endothermic or exothermic based on their heat exchange with the surroundings. Endothermic reactions absorb heat, while exothermic reactions release heat. The temperature dependence of the equilibrium constant K is influenced by the nature of the reaction; for endothermic reactions, increasing temperature increases K, while for exothermic reactions, it decreases K.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It provides insight into the extent of a reaction and how it shifts in response to changes in conditions. Understanding how K varies with temperature is crucial for predicting the direction of a reaction's shift when temperature changes.

(c) In each case, indicate whether K should increase or decrease with increasing temperature. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)