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?

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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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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Consider the reaction: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.

T (K) [N₂] [H₂] [NH₃] K_c

500 0.115 0.105 0.439 _

575 0.110 _ 0.128 9.6

775 0.120 0.140 _ 0.0584

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Consider the following reaction: H₂(g) + I₂(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.

T (°C) [H₂] [I₂] [HI] Kc

25 0.0355 0.0388 0.922 _

340 _ 0.0455 0.387 9.6

445 0.0485 0.0468 _ 50.2

Textbook Question

Consider the reaction:

2 NO( g) + Br2( g)Δ2 NOBr( g) Kp = 28.4 at 298 K

In a reaction mixture at equilibrium, the partial pressure of NO is 125 torr and that of Br2 is 148 torr. What is the partial pressure of NOBr in this mixture?