Part A Calculating Equilibrium Constants The equilibrium 1 constant, K, of a rea

Question

Part A Calculating Equilibrium Constants The equilibrium 1 constant, K, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. Phosgene (carbonyl chloride, Cole, 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 coe+ Ch(8) COC, (g ) Carbon monoxide and chiorine gas are allowed to react in a sealed vessel at 487 "C. At equilibrium, the concentrations were measured and the folowing results obtained For a gaseous reaction with the general form aA+ bB C+ dD the K, and K, expressions are given by Partial Pressure Gas (atm) COO C1, 1.22 COC, 0.270 K, A PR what is the equilibrium constantKp, of this reaction? Express your answer numerically. Hints PP The subscript corp indicates whether Kis 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 throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change the sample remain pure. The concentration is effectively equal to 1, and will not impact the magnitude of K. He as n o o on ? Submit My Answers Give Up Deriving concentrations from data In Part A, you were given the equilibrium pressures, which could be plugged crectly into the formula for K. In Part B howeveryou will be given initial concentrations and only one equinbrum concentrationYou must use this data to find all three equilibrium concentrations before you can apply the formula for K. Part B The following reaction was performed in a sealed vessel at 780 °C: (e) + I (g) 2HI(R) Initially, only H, and I, were present at concentrations of (Hy] = 3.60 M and (2) = 2.10M . The equilibrium concentration of I, is 0.0700 M. What is the equilibrium constantK, for the reaction at this temperature? Express your answer numerically. Hints DVD AND no o a ?

Explanation / Answer

part A)

Kp = (PCOCl2) / (PCO) (PCl2)

Kp = (0.270) / (0.880)(1.22)

Kp = 0.270 / 1.0736

Kp = 0.251

part B) Kc = [HI]2 / [H2][I2]

initially

[H2] = 3.60 M

[I2] = 2.10 M

at equilibrium

[I2] = 0.070 M

2.10 - 0.070 = 2.03 M I2 consumed

[H2] = 3.60 - 2.03 = 1.57 M

[HI] = 2.03 x 2 = 4.06 M

Kc = [4.06]2 / [1.57][0.07]

Kc = 16.4836 / 0.1099

Kc = 149.98

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