At 700 K, the equilibrium constant for the reaction CCl 4 (𝑔) ⇌ C(𝑠) + 2 Cl 2 (𝑔) is 𝐾 𝑝 = 0.76. A flask is charged with 2.00 atm of CCl 4 , which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl 4 and Cl 2 at equilibrium?

Step 1: Write the balanced chemical equation for the reaction: CCl_{4}(g) ⇌ C(s) + 2 Cl_{2}(g).. Step 2: Define the initial pressures of the reactants and products. Initially, the pressure of CCl_{4} is 2.00 atm, and the pressures of C(s) and Cl_{2} are 0 atm.. Step 3: Let the change in pressure of CCl_{4} at equilibrium be -x atm. Since C(s) is a solid, its pressure does not contribute to the equilibrium expression. The change in pressure of Cl_{2} will be +2x atm.. Step 4: Write the expression for the equilibrium constant, K_{p}, in terms of the partial pressures of the gases at equilibrium. K_{p} = (P_{Cl2}$$)^2 / P$$_{CCl4}.. Step 5: Substitute the expressions for the pressures at equilibrium into the K_{p} expression and solve for x. Use the quadratic formula if necessary to find the value of x, and then calculate the equilibrium partial pressures of CCl_{4} and Cl_{2}.

At 700 K, the equilibrium constant for the reaction CCl4(𝑔) ⇌ C(𝑠) + 2 Cl2(𝑔) is 𝐾𝑝 = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl4 and Cl2 at equilibrium?

Step 1: Write the balanced chemical equation for the reaction: CCl_{4}(g) ⇌ C(s) + 2 Cl_{2}(g). Step 2: Define the initial pressures of the reactants and products. Initially, the pressure of CCl_{4} is 2.00 atm, and the pressures of C(s) and Cl_{2} are 0 atm. Step 3: Let the change in pressure of CCl_{4} at equilibrium be -x atm. Since C(s) is a solid, its pressure does not contribute to the equilibrium expression. The change in pressure of Cl_{2} will be +2x atm. Step 4: Write the expression for the equilibrium constant, K_{p}, in terms of the partial pressures of the gases at equilibrium. K_{p} = (P_{Cl2}$$)^2 / P$$_{CCl4}. Step 5: Substitute the expressions for the pressures at equilibrium into the K_{p} expression and solve for x. Use the quadratic formula if necessary to find the value of x, and then calculate the equilibrium partial pressures of CCl_{4} and Cl_{2}.

Ch.15 - Chemical Equilibrium

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경

모든 교과서

Brown 14th Edition

Ch.15 - Chemical Equilibrium

문제 89b

15장, 문제 89b

At 700 K, the equilibrium constant for the reaction CCl₄(𝑔) ⇌ C(𝑠) + 2 Cl₂(𝑔) is 𝐾_𝑝= 0.76. A flask is charged with 2.00 atm of CCl₄, which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl₄ and Cl₂ at equilibrium?

검증된 단계별 안내

Step 1: Write the balanced chemical equation for the reaction: CCl₄(g) ⇌ C(s) + 2 Cl₂(g).

Step 2: Define the initial pressures of the reactants and products. Initially, the pressure of CCl₄ is 2.00 atm, and the pressures of C(s) and Cl₂ are 0 atm.

Step 3: Let the change in pressure of CCl₄ at equilibrium be -x atm. Since C(s) is a solid, its pressure does not contribute to the equilibrium expression. The change in pressure of Cl₂ will be +2x atm.

Step 4: Write the expression for the equilibrium constant, K_p, in terms of the partial pressures of the gases at equilibrium. K_p = (P_Cl₂)^2 / P_CCl₄.

Step 5: Substitute the expressions for the pressures at equilibrium into the K_p expression and solve for x. Use the quadratic formula if necessary to find the value of x, and then calculate the equilibrium partial pressures of CCl₄ and Cl₂.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

11m

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 CCl₄(g) ⇌ C(s) + 2 Cl₂(g), Kp = 0.76 indicates that at equilibrium, the ratio of the pressure of Cl₂ squared to the pressure of CCl₄ is constant. This concept is crucial for determining the concentrations or pressures of reactants and products at equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. In this case, if the initial pressure of CCl₄ is altered, the system will shift to either produce more products or reactants to re-establish equilibrium, which is essential for calculating the final partial pressures.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In the context of the given reaction, understanding how to calculate the partial pressures of CCl₄ and Cl₂ at equilibrium is necessary to solve the problem, as it involves using the initial conditions and the equilibrium constant.