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Consider the reaction:
[Co(NH3)5Cl]2+(aq) + [Co(CN)5]3(aq) [Co(CN)5Cl]3(aq) + Co2+(aq) + 5 NH3(aq)
The initial concentration of each reactant is equal to the eigthth and ninth digits of your Student ID Number divided by 105 M = Cinit. At some temperature, after 12 s, the concentrations of each reactant are reduced to 0.93×Cinit.
What is the average rate of reaction for the first 12 s in terms of the loss of [Co(CN)5]3?
What is the average rate of reaction for the first 12 s in terms of the gain of NH3?
The rate law at 25 oC is found to be Rate = k[Co(NH3)5Cl2+] [Co(CN)53] with k=5×107 M1s1. What is the initial rate at 25 oC?
Turn in the following on a clean, full sheet of paper (not torn out of a notebook):
Student ID Number
The answers to questions a, b, and c. Show your work.