I have answer to part A! Only answer Part B Deriving concentrations from data In

Question

I have answer to part A! Only answer Part B

Deriving concentrations from data 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. Part B The following reaction was performed in a sealed vessel at 746 degree C : H2 (g) + I2(g) 2HI(g) Initially, only H2 and 12 were present at concentrations of [H2] = 3.30M and [I2] = 2.45M. The equilibrium concentration of I2 is 0.090CM. What is the equilibrium constant, K, for the reaction at this temperature? Express your answer numerically. Part A Phosgene (carbonyl chloride), COCl2, s an extremely toxic gas that is used n 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 467 degree C . At equilibrium, the concentrations were measured and the following results obtained: What is the equilibrium constant, K, of this reaction?

Explanation / Answer

           H2 +    I2 <------------------> 2HI

            at initial         3.3      2.45                      0

At equilibrium 3.3- x   2.45 - x              2x

                                            from data 2.45 - x= 0.09

                                                               x= 2.36

[H2 ]=3.3- x =0.94

[I2]= 2.45 - x= 0.09

[HI]= 2x = 4.72

Kc = [HI]2/[H2 ]/[I2]

       = (4.72)2/ 0.09x0.94

     = 263.33

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