Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91*10^3 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 117 torr and that of Cl2 is 205 torr. What is the partial pressure of SO2Cl2 in this mixture?

검증된 단계별 안내

Identify the given equilibrium reaction: \( \text{SO}_2\text{Cl}_2(g) \rightleftharpoons \text{SO}_2(g) + \text{Cl}_2(g) \).

Write the expression for the equilibrium constant \( K_p \) for the reaction: \( K_p = \frac{P_{\text{SO}_2} \cdot P_{\text{Cl}_2}}{P_{\text{SO}_2\text{Cl}_2}} \).

Substitute the given values into the \( K_p \) expression: \( K_p = 2.91 \times 10^3 \), \( P_{\text{SO}_2} = 117 \text{ torr} \), \( P_{\text{Cl}_2} = 205 \text{ torr} \).

Rearrange the equation to solve for \( P_{\text{SO}_2\text{Cl}_2} \): \( P_{\text{SO}_2\text{Cl}_2} = \frac{P_{\text{SO}_2} \cdot P_{\text{Cl}_2}}{K_p} \).

Calculate \( P_{\text{SO}_2\text{Cl}_2} \) using the rearranged equation and the given values.

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주요 개념

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

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium for a given reaction at a specific temperature. For the reaction SO2Cl2(g) ⇌ SO2(g) + Cl2(g), Kp is calculated using the formula Kp = (P_SO2 * P_Cl2) / P_SO2Cl2, where P represents the partial pressures of the gases involved.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. It can be determined using Dalton's Law, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual components. In this case, the partial pressures of SO2 and Cl2 are given, and the partial pressure of SO2Cl2 can be derived from the equilibrium constant.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. In the context of this reaction, if the concentrations or pressures of the reactants or products are altered, the equilibrium will shift to favor the formation of either the reactants or products, affecting the partial pressures involved.