If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3...

If the rate law for the clock reaction is: Rate = k [ I-] [ BrO3 -] [H+] A clock reaction is run with the following initial concentrations: [I-] [BrO3-] [H+] [S2O32-] 0.002 0.008 0.02 0.0001 The reaction time is 28 seconds Calculate k in the rate law:

Also:

Rate = k [ I-] [ BrO3 -] [H+] A clock reaction is run at 19 ºC with the following initial concentrations [I-] [BrO3-] [H+] [S2O32-] 0.002 0.008 0.02 0.0001 Then the experiment is repeated at 33 ºC, the rate constant k is found to be 2.7 times larger. Calculate the activation energy

Expert Solution

queen_honey_blossom answered 2 years ago

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