Question

The following data were obtained for the chemical reaction: A + B ---> products Exp. Initial...

The following data were obtained for the chemical reaction: A + B ---> products

Exp. Initial A
(mol/L)		 Initial B
(mol/L)		 Init. Rate of Formation
of products (M s-1)
1 0.040 0.040 9.6 x 10-6
2 0.080 0.040 1.92 x 10-5
3 0.080 0.020 9.6 x 10-6

(a) Determine the rate law for this reaction.
(b) Find the rate constant.
(c) What is the initial rate of reaction when [A]o = 0.12 M and [B]o = 0.015

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Homework Answers

Answer #1

a)

see experiment 1 and 2:

[A] doubles

[B] is constant

rate doubles

so, order of A is 1

see experiment 3 and 2:

[A] is constant

[B] doubles

rate doubles

so, order of B is 1

overall order = 1 + 1 = 2

Rate law is:

rate = k*[A]*[B]

b)

Put values from 1st row of table in rate law

rate = k*[A]*[B]

9.6*10^-6 = k*0.04*0.04

k = 0.00600 M-1.s-1

Answer: 0.00600 M-1.s-1

c)

rate =0.006*0.12*0.015

rate = 1.08*10^-5 M/s

Answer: 1.08*10^-5 M/s

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