Question

Given the initial rate data for the reaction A + B → C, determine the rate...

Given the initial rate data for the reaction A + B → C, determine the rate expression for the reaction.

[A], M

[B], M

Δ[C]/Δt (initial) M/s

0.0500

0.160

2.24 ´ 10-3

0.0750

0.160

3.36 ´ 10-3

0.0750

0.272

9.72 ´ 10-3
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Homework Answers

Answer #1

Let the rate expression be Rate = k[A]x[B]y.

we need to find out the values of k,x and y.

from first set,

2.24*10-3 = k[0.0500]x[0.160]y ....(1)

Similarly,

3.36*10-3 = k[0.0750]x[0.160]y ....(2)

9.72*10-3 =k[0.0750]x[0.272]y ...(3)

Dividing eq 2 by 1 we get-

3.36*10-3/2.24*10-3 = [0.0750]x[0.0160]y / [0.0500]x[0.160]y

1.5 = [0.0750]x/[0.0500]x

1.5 = [1.5]x

[1.5]1 = [1.5]x

x = 1

Now dividing eqn 3 by eqn 2-

9.72*10-3/3.36*10-3 = [0.0750]x[0.272]y / [0.0750]x[0.160]y

2.89 = [1.7]y

[1.7]2 = [1.7]y

y = 2

so, Rate = k[A][B]2

k = Rate/[A][B2]

keeping values in this-

k = 2.24*10-3/0.0500*(0.160)2 = 1.75

k = 3.36*10-3/0.0750*(0.160)2 = 1.75

so,

Rate = 1.75[A][B]2

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