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 + bB 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 gas that is used in manufacturing certain dyes and plastics. Phosgene can be produced by reacting carbon monoxide and chlorine gas at high temperatures: Carbon monoxide and chlorine gas are allowed to react in a sealed vessel at 463 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. 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 796 degree C: H2(g) + I2(g) 2HI(g) Initially, only H2 and I2 were present at concentrations of [H2] = 3.00 M an d [I2] = 2.25 M. The equilibrium concentration of I2 is 0.0700 M. What is the equilibrium constant, Kc, for the reaction at this temperature? Express your answer numerically Kc =

Explanation / Answer

We Know that :      The given Reaction is :         CO ( g)   + Cl2 ( g ) <----------> COCl2 ( g )               Kp   =   PCOCl2 / PCO x PCl2                         = 0.280 / 0.730 x 1.30                          = 0.295 b.               The given Reaction is :            H2 ( g )   + I2 ( g) <------> 2 HI ( g )     I       3.0M           2.25M                 0      C      -x                 -x                    + 2 x       E    3.0 -x           2.25 -x                 2 x             Given that the equilibrium concentration of I2is 0.070 M                2.25 - x = 0.070                     x = 2.18 M                                                         Kc = [ HI ]2 /  [ H2 ] [ I2 ]                                                                  = [ 4.36 ]2 / [ 0.070 ] [ 0.82 ]                                                                   = 331.177

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