Question

The following data was measured for the reaction above at a constant temperature.

Experiment Initial [A] mol L‐1 Initial [B] mol L‐1 Initial rate of formation of C (mol L‐1 s‐1)
1 0.10 0.10 1.12 x 10‐3
2 0.10 0.20 2.24 x 10‐3
3 0.20 0.10 4.48 x 10‐3

What is the order of the reaction with respect to A?
What is the order of the reaction with respect to B?
What is the rate law for this reaction?
Calculate the rate constant.

Answer 1

A is second order

B is first order.

`V=k[A]^(2) [B]`

`k=1.12`

Step-by-step explanation:

order of the reaction with respect to A

`\frac{[A]_(3)}{[A]_1{}} =2`

`\frac{[V]_(3)}{[V]_1{}} =4`

Then V∝
`[A]^(2)`

order of the reaction with respect to B

`\frac{[B]_(2)}{[B]_1{}} =2`

`\frac{[V]_(2)}{[V]_1{}} =2`

Then V∝
`[B]}`

Rate law of the reaction

`V=k[A]^(2)[B]`

Rate constante of the reaction

`k=(V)/([A]^(2)[B])`

`k=1.12`