Open Question
Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kc = 102 at 500 K. If a reaction mixture initially contains 0.110 M CO and 0.110 M H2O, what will the equilibrium concentration of each of the reactants and products be?
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 59
Consider the reaction: Br2(g) + Cl2(g) ⇌ 2BrCl(g) with Kp = 1.11 * 10^-4 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 735 torr at 150 K. Calculate the equilibrium partial pressure of BrCl.
Verified step by step guidance1
Identify the initial conditions: The initial partial pressures are 755 torr for Br2 and 735 torr for Cl2.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in partial pressures as the system reaches equilibrium. Let x be the change in pressure for Br2 and Cl2, and 2x for BrCl.
Write the expression for the equilibrium constant Kp: \( K_p = \frac{{(P_{\text{BrCl}})^2}}{{P_{\text{Br}_2} \cdot P_{\text{Cl}_2}}} \).
Substitute the equilibrium expressions from the ICE table into the Kp expression: \( K_p = \frac{{(2x)^2}}{{(755 - x)(735 - x)}} \).
Solve the equation for x, which represents the change in pressure, and use it to find the equilibrium partial pressure of BrCl, which is 2x.
Related Practice
Textbook Question
Consider the reaction: HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Kc = 1.8⨉10-5 at 25°C If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 °C?
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Textbook Question
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99⨉10-7 at 227 °C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?
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Textbook Question
Consider the reaction: A(g) ⇌ B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. b. Kc = 0.010
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Open Question
Consider the reaction: A(g) ⇌ 2B(g). Find the equilibrium partial pressures of A and B for each value of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions. a. Kp = 1.0 b. Kp = 1.0 × 10^-4 c. Kp = 1.0 × 10^5.
Open Question
Consider this reaction at equilibrium: CO(g) + Cl2(g) ⇌ COCl2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. COCl2 is added to the reaction mixture. b. Cl2 is added to the reaction mixture. c. COCl2 is removed from the reaction mixture.