The equilibrium constant, K, of a reaction at a particular temperature is determ

Question

The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA + 6B cC + dD the Kc and Kp expressions are given by The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved in the reaction. In Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initial concentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K. The following reaction was performed in a sealed vessel at 794 degree C : Initially, only H2 and I2 were present at concentrations of [H2] = 3.30M and [I2] = 2.10M. The equilibrium concentration of I2 is 0.0600 M What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically. The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA + 6B cC + dD the Kc and Kp expressions are given by The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved in the reaction. Phosgene (carbonyl chloride), COCl2, is an extremely toxic used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: CO(g) + Cl2(g) COCl2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 471 degree C. At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, Kp, of this reaction? Express your answer numerically. Now consider the reaction for which in the initial mixture Is the reaction at equilibrium? If not, in which direction will it proceed to reach equilibrium? The reaction is already at equilibrium. The reaction will proceed in reverse to form reactants. The reaction will proceed forward to form products.

Explanation / Answer

Make the "ICE" chart: I stands for initial concentration or pressure, C for change in conc./press. and E for equilibrium state H2 + I2 2HI I :: 3.3M 2.10M 0 (Since it is not mentioned in question, it will be 0) C:: -X -X +2X ( here, since there are more reactants than product, the change in concentration is -X; coeff. goes in front of the X if there is one like the 2HI its +2X) E:: 3.3 - X 2.10- X = .060+2(x) to find X; 2.1 - .06 = X therefore, X = 2.04 now after you plug back in, you will get 1.26 for H2 4.08 for 2HI and as given, .06 for I2 Now for Kc : (Product) raised to power of coeff. divided by Reactant raised to each of its coeff. = (4.08)^2 divided by (1.26)^1 * (.06)^1 = Kc = 220.19

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