a) rate law for the reaction b) rate constant k I attached my work how I solved

Question

a) rate law for the reaction b) rate constant k

I attached my work how I solved this problem can you please help me with:

1) If my calculations are correct (if not please help me where I made the mistake)

2) I am really confused about the units for rate constant k. I have 1/M*s. is this correct?

Consider the equation: CHC13(g) +Cl2(g) -CCI4(g) + HCI(g) The initial rate of reaction is measured at several different concentrations of the reactants with the following results: [CHCl3] (M) 0.010 0.020 0.020 0.040 [Cl2l (M) 0.010 0.010 0.020 0.040 Initial Rate (M/s) 0.0035 0.0069 0.0098 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction

Explanation / Answer

A.I guess the part A question is solved according the concept .

rate law = K [CHCl3] [CL2]2

I guess all ur questions are correct with their solutions

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