A + B → C Select the rate law for the reaction above using the following information: Holding the concentration of A constant and doubling the concentration of B results in the rate of the reaction increasing from 1.5E-3 M/s to 1.2E-2 M/s. Keeping the concentration of B constant and doubling A results in the rate of the reaction increasing from 1.5E-3 M/s to 3.0E-3 M/s.

Question

Israel Huff

Chemistry

20 February, 03:04

A + B → C Select the rate law for the reaction above using the following information: Holding the concentration of A constant and doubling the concentration of B results in the rate of the reaction increasing from 1.5E-3 M/s to 1.2E-2 M/s. Keeping the concentration of B constant and doubling A results in the rate of the reaction increasing from 1.5E-3 M/s to 3.0E-3 M/s.

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Darrell Gillespie · Answer 1

For the initial conditions:

1.5E-3 = k A^n B^m

For the second condition:

1.2E-2 = k A^n (2B) ^m

1.2E-2 = 2^m k A^n B^m

From the initial condition:

1.2E-2 = 2^m (1.5E-3)

m = 3.32

For the third condition:

3.0E-3 = k (2A) ^n B^m

3.0E-3 = 2^n k A^n B^m

3.0E-3 = 2^n (1.5E-3)

n = 1

Therefore, the rate law is:

r = k A B^3.32