Question

estion 15 of 16 > Using the data in the table, calculate the rate constant of this reaction Trial Rate (M/s) 0.0230 1 [A] (M) 0.320 0.320 0.416 [B] (M) 0.390 0.936 0.390 2 0.132 A+B — C+D 0.0299 Units ku

Answer 1

see experiment 1 and 2:

[A] becomes 0.416/0.320 = 1.3 times

[B] is constant

rate becomes 0.0299/0.0230 = 1.3 times

so, order of A is 1

see experiment 1 and 2:

[A] is constant

[B] becomes 0.936 / 0.390 = 2.4 times

rate becomes 0.132/0.0230 = 5.76 times

Since 2.4^2 = 5.76, order of B is 2

Rate law is:

rate = k*[A]*[B]^2

Put values from 1st row of table in rate law

rate = k*[A]*[B]^2

2.3*10^-2 = k*0.32*0.39^2

k = 0.4726 M-2.s-1

Answer:

K = 0.473

Units = M-2.s-1