Question

The rate expression for a particular reaction is rate = k[A][B]2.If the initial concentration of B is increased from 0.1 M to 0.3 M, the initial rate will increase by which of the following factors? 9 3 2 6 12

Answer 1

The initial rate of the reaction increases by a factor of 9 when the concentration of B is increased from 0.1 M to 0.3 M, due to the squared dependence on B's concentration in the rate expression.

Step-by-step explanation:

The rate expression for a particular reaction is rate = k[A][B]^2. When the initial concentration of B is increased from 0.1 M to 0.3 M, we must consider the change in the rate with respect to the concentration of B. Since the rate law indicates that the rate is proportional to the concentration of B squared ([B]^2), a change in [B] has a squared effect on the rate.

If the initial concentration of B is increased by a factor of three (from 0.1 M to 0.3 M), the initial rate will increase by a factor of three squared, because the rate is proportional to [B]^2. Therefore, the rate increases by 3^2, which is 9. The initial rate will increase by a factor of 9.

Answer 2

Increasing the initial concentration of B from 0.1 M to 0.3 M in the reaction with a rate expression of rate = k[A][B]^2 will increase the initial reaction rate by a factor of 9.

Step-by-step explanation:

The rate expression given is rate = k[A][B]2. This indicates that the reaction rate depends on the concentration of A and the square of the concentration of B. An increase in the concentration of B from 0.1 M to 0.3 M means that the concentration of B is tripled.

According to the rate expression, if we triple the concentration of B, the effect on the rate will be the square of this factor because the rate is proportional to the square of the concentration of B (B squared). Therefore, the rate will increase by a factor of 32, which is 9. So, the initial rate of the reaction will increase by a factor of 9.