(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 0.221 M and that of C2O42-(aq) is 0.345 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 0.161 0.161 4.38e-05 2 0.161 0.322 0.000175 3 0.322 0.161 8.76e-05 4 0.322 0.322 0.000351

Explanation / Answer

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

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

K = 0.000351 / (0.322)(0.322)2

K = 0.000351 / 0.0334

K = 0.010 M-2s-1

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

rate = 0.010 [0.221][0.345]2

rate = 2.63 x 10-4 M/s

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