Question

Consider the reaction A ⟶Products

Use the following rate data to determine the order of the reaction with respect to the reactant A.

     [A] (M)               Initial Rate (M/s)

     0.10           0.015

     0.40           0.060

1

0

3

2

Answer 1

The given reaction is A---> products

Trial-1: The initial concentration of A is 0.10 M when the initial rate is 0.015 M/s

Trial-2: The initial concentration of A is 0.40 M when the initial rate is 0.060 M/s

Let the order be m

Rate law for first trial will be:
`0.015M/s = k.[0.10M]^(m)`

Rate law for second trial will be:
`0.060M/s = k.[0.40M]^(m)`

Rate- 2/ Rate-1 :
`(0.060M/s)/(0.0150M/s)=(k(0.40)^(m))/(k.(0.10)^(m))`

`4 = 4^(m)`

So, m = 1

Therefore the order of the reaction is 1