The following set of data was obtained by the method of initial rates for the re

Question

The following set of data was obtained by the method of initial rates for the reaction:

(H3C)3CBr + OH- ? (H3C)3COH + Br-

What is the value of the rate constant, k? [(H3C)3CBr], M [OH-] M Initial Rate M/s 0.25 0.25 1.1x10e-4 0.25 0.252.2x10e-4 0.25 0.50 2.2x10e-4 Please show step by step
The following set of data was obtained by the method of initial rates for the reaction:

(H3C)3CBr + OH- ? (H3C)3COH + Br-

What is the value of the rate constant, k? [(H3C)3CBr], M [OH-] M Initial Rate M/s 0.25 0.25 1.1x10e-4 0.25 0.252.2x10e-4 0.25 0.50 2.2x10e-4 Please show step by step
The following set of data was obtained by the method of initial rates for the reaction:

(H3C)3CBr + OH- ? (H3C)3COH + Br-

What is the value of the rate constant, k? [(H3C)3CBr], M [OH-] M Initial Rate M/s 0.25 0.25 1.1x10e-4 0.25 0.252.2x10e-4 0.25 0.50 2.2x10e-4 Please show step by step
The following set of data was obtained by the method of initial rates for the reaction:

(H3C)3CBr + OH- ? (H3C)3COH + Br-

What is the value of the rate constant, k? [(H3C)3CBr], M [OH-] M Initial Rate M/s 0.25 0.25 1.1x10e-4 0.25 0.252.2x10e-4 0.25 0.50 2.2x10e-4 Please show step by step

Explanation / Answer

rate = k*([(H3C)3CBr]^a)*([OH-]^b)

when [(H3C)3CBr is doubled, keeping [OH-] constant, rate gets doubled => rate is directly proportional to [(H3C)3CBr.

Similarly, when [OH-] is doubled, keeping [(H3C)3CBr]] constant, rate gets doubled => rate is directly proportional to [OH-]

=>.a = 1 and b = 1

=> rate =k*([(H3C)3CBr])*([OH-])

Now, we have, rate 1.1*10^-4, [OH-] = 0.25 [(H3C)CBr] = 0.25

=> k = (1.1*10^-4)/(0.25*0.25)

=> k = 0.00176 M^-1s^-1

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