The equilibrium 2 NO(π) + Cl2(π) β 2 NOCl(π) is established at 500.0 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate πΎπ for this reaction at 500.0 K.
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Identify the balanced chemical equation: 2 NO(g) + Cl_2(g) β 2 NOCl(g).
Write the expression for the equilibrium constant K_p for the reaction: K_p = (P_NOCl^2) / (P_NO^2 * P_Cl2).
Substitute the given equilibrium partial pressures into the K_p expression: P_NO = 0.095 atm, P_Cl2 = 0.171 atm, and P_NOCl = 0.28 atm.
Calculate the numerator of the K_p expression: (P_NOCl)^2.
Calculate the denominator of the K_p expression: (P_NO)^2 * P_Cl2.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Chemical Equilibrium
Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations of the substances involved.
The equilibrium constant, Kp, is a numerical value that expresses the ratio of the partial pressures of the products to the partial pressures of the reactants at equilibrium, each raised to the power of their coefficients in the balanced equation. For the reaction 2 NO(g) + Cl2(g) β 2 NOCl(g), Kp is calculated using the formula Kp = (P_NOCl^2) / (P_NO^2 * P_Cl2), where P represents the partial pressures of the gases.
Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In equilibrium calculations, knowing the partial pressures of each gas allows for the determination of the equilibrium constant.
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