(a) What is the rate law for this reaction? Rate = k [HgCl 2 (aq)] [C 2 O 4 2- (

Question

(a) What is the rate law for this reaction?

Rate = k [HgCl2(aq)] [C2O42-(aq)]

Rate = k [HgCl2(aq)]2 [C2O42-(aq)]     

Rate = k [HgCl2(aq)] [C2O42-(aq)]2

Rate = k [HgCl2(aq)]2 [C2O42-(aq)]2

Rate = k [HgCl2(aq)] [C2O42-(aq)]3

Rate = k [HgCl2(aq)]4 [C2O42-(aq)]

(b) What is the value of the rate constant?





(c) What is the reaction rate when the concentration of HgCl2(aq) is 0.302 M and that of C2O42-(aq) is 0.546 M if the temperature is the same as that used to obtain the data shown above?

M/s

Experiment [HgCl2(aq)] (M) [C2O42-(aq)] (M) Rate (M/s) 1 0.194 0.194 8.25e-05 2 0.194 0.388 0.000330 3 0.388 0.194 0.000165 4 0.388 0.388 0.000660

Explanation / Answer

a) Rate = k [HgCl2(aq)] [C2O42-(aq)]2

b) K = rate / [HgCl2(aq)] [C2O42-(aq)]2

K = 0.00033 / (0.194)(0.388)2

K = 0.00033 / 0.0292

K = 0.0113 M-2 s-1

C) rate = (0.0113) (0.302) (0.546)2

rate = 1.017 x 10-3 M/s

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