Question

has an initial rate of 0.0300 M / s. 0.0300 M/s. What will the initial rate be if [ A ] [A] is halved and [ B ] [B] is tripled?

Answer 1

The initial rate is 0.135 m/s.

Step-by-step explanation:

Given that,

Rate = 0.0300 m/s

`[A]=([A])/(2)`

`[B]=3[B]`

Suppose, The rate is,

`\text{rate}=k[A][B]^2`

We need to calculate the initial rate

Using formula of rate

`rate=k[A][B]^2`

Put the value A and B

`rate=k*([A])/(2)[3B]^2`

`rate=k*([A])/(2)[9B^2]`

`rate=4.5k[A][B]^2`

`rate =4.5*0.0300`

`rate=0.135\ m/s`

Hence, The initial rate is 0.135 m/s.

Answer 2

0.135M/s

Step-by-step explanation:

We are given that

Initial rate of reaction=0.0300M/s

We have to find the initial rate if [A] is halved and [B] is tripled.

Initial rate,
`Rate=k[A][B]^2`=0.0300M/s

`[A]'=(1)/(2)[A]`

`[B]'=3[B]`

New, initial rate=
`k[A]'[B]'^2`

Substitute the values then we get

New, initial rate,Rate=
`k* (1)/(2)[A]* (3[B])^2`

New, initial rate

Rate=
`4.5k[A][B]`

New initial rate=
`4.5* 0.0300=0.135M/s`

Hence, the initial rate will be 0.135M/s when [A] is halved and [B] is tripled.