Problem: The following data were obtained for the hypothetical reaction 2A + B → products.[A]0 (M)[B]0 (M)Initial Rate (M/s)10.20.1520.20.22030.60.145What is the overall order of this reaction?A) 3B) 1/2C) 0D) 4E) 1

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We’re being asked to calculate the overall order of this hypothetical reaction:

2A + B → products

Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


We’re going to calculate the overall order for the reaction:

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Problem Details

The following data were obtained for the hypothetical reaction 2A + B → products.


[A]0 (M)

[B]0 (M)

Initial Rate (M/s)

1

0.2

0.1

5

2

0.2

0.2

20

3

0.6

0.1

45


What is the overall order of this reaction?

A) 3

B) 1/2

C) 0

D) 4

E) 1