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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

Respuesta :

Chlidonias

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: [tex]0.015M/s = k.[0.10M]^{m}[/tex]

Rate law for second trial will be:  [tex]0.060M/s = k.[0.40M]^{m}[/tex]

Rate- 2/ Rate-1 : [tex]\frac{0.060M/s}{0.0150M/s}=\frac{k(0.40)^{m}}{k.(0.10)^{m}}[/tex]

[tex]4 = 4^{m}[/tex]

So, m = 1

Therefore the order of the reaction is 1



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