The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products equilibrium. For a gaseous reaction with the general form aA+bB cC + dD the K, and K, expressions are given by K₂ = K₂ = [C] [D] [A] [B] (Pc) (Pb) (PA) (PB) 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 since their composition does not change The standard state of Part A Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is 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) = COCk₂2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 460 °C. At equilibrium, the concentrations were measured and the following results obtained: Gas CO Ch₂ COC₂ What is the equilibrium constant, K₂, of this reaction? Express your answer numerically. View Available Hint(s) Partial Pressure (atm) 0.810 1.14 0.270
The equilibrium constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products equilibrium. For a gaseous reaction with the general form aA+bB cC + dD the K, and K, expressions are given by K₂ = K₂ = [C] [D] [A] [B] (Pc) (Pb) (PA) (PB) 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 since their composition does not change The standard state of Part A Phosgene (carbonyl chloride), COCl2, is an extremely toxic gas that is 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) = COCk₂2(g) Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 460 °C. At equilibrium, the concentrations were measured and the following results obtained: Gas CO Ch₂ COC₂ What is the equilibrium constant, K₂, of this reaction? Express your answer numerically. View Available Hint(s) Partial Pressure (atm) 0.810 1.14 0.270
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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