The reaction has an initial rate of 0.0300 M/s.

A+B YIELDS C+D rate=k[A][B]^2

What will the initial rate be if [A] is halved and [B] is tripled? (answer) M/s

What will the initial rate be if [A] is tripled and [B] is halved? answer M/s

The initial rate if [A] is halved and [B] is tripled is 0.135

The initial rate if [A] is tripled and [B] is halved is 0.0225

Explanation:

You have:

If [A] is halved and [B] is tripled, the new concentrations are:

Replacing these new concentrations in the velocity expression:

Replacing k*[A]*[B]² with 0.0300 m/s:

The initial rate if [A] is halved and [B] is tripled is 0.135

If [A] is tripled and [B] is halved, the new concentrations are:

Replacing these new concentrations in the velocity expression:

Replacing k*[A]*[B]² with 0.0300 m/s:

The initial rate if [A] is tripled and [B] is halved is 0.0225