Question

In: Chemistry

Determine the integrated form of the third-order rate law of the form: -d[A]/dt = k[A]^3. Starting...

Determine the integrated form of the third-order rate law of the form:

-d[A]/dt = k[A]^3.

Starting from a 0.5 M initial concentration of A, and a rate constant of 0.1 M^-2 * s^-1, how much time would be required before reaching a 0.3M concentration of A?

Answer Options

78.2 s

35.6 s

22.3 s

13.7 s

Solutions

Expert Solution

Given rate law is :   -d[A]/dt = k[A]3

                             d[A]/[A]3 = -kdt

                     apply integration we get

                           d[A]/[A]3 = - kdt

                              -(1/(2[A]2 )) = -kt + I                           I = integration constant

Obtaining the value of I :

If [Ao] be the initial concentration.

When t= 0 s ---> [A] = [Ao] then above equation becomes     -(1/(2[Ao]2 )) = -k(0) + I  

                                                                                                        I = -(1/(2[Ao]2 ))

Therefore the integration equation is     -(1/(2[A]2 )) = -kt + -(1/(2[Ao]2 ))

       kt = (1/(2[A]2 )) -(1/(2[Ao]2 ))  

kt = (1/2) [(1/[A]2) - (1/[Ao]2)]

Given [Ao] = 0.5 M

[A] = 0.3M

k = rate constant = 0.1 M-2 s-1

Plug the values we get

t = (1/2k) [(1/[A]2) - (1/[Ao]2)]

t = (1/(2x0.1)) [(1/0.32) - (1/0.52)]

= 35.6 s

Therefore the required time is 35.6 s

                     


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