Question

For a reaction the initial rate is given as R0=k(A) 2(B) by what factor ,the initial rate of reaction will increase if initial concentration of A is taken 1.5 times and B is tripled​

Answer 1

Answer: The rate will increase 6.75 times of initial rate.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$Rate=k[A]^x[B]^y$

k= rate constant

x = order with respect to A

y = order with respect to A

Given: Rate law, $R_0=k[A]^2[B]^1$, order with respect to A is 2, order with respect to B is 1.

Thus when initial concentration of A is taken 1.5 times and B is tripled​:

Rate law=$R=k[1.5\times A]^2[3\times B]^1$

$R=k[1.5]^2[A]^2[3]^1[B]^1$

$R=k\times 6.75\times [A]^2[B]^1$

$R=6.75\times R_0$

Thus the rate will increase 6.75 times of initial rate.