A reaction is first order in A and second order in B:How is the rate affected when the concentration of both A and B are doubled?

A reaction is first order in A and second order in B:How is the rate affected on increasing the concentration of B three times?

For the reaction A + 2B to C, the reaction rate is doubled if the concentration of A is doubled , the rate is increased by four times when concentrations of both A and B are increased by four times . The order of the reaction is _______.

A reaction is first order with respect to reactant A and second order with respect to reactant B. The rate law for the reaction is given by

What are the units for rate constants for zero order and second order reactions if time is expressed in seconds and concentration of reactants in mol//L ?

How do half-lives of the first order and zero order reactions change with initial concentration of reactants?

In a first-order reaction A rarr B , if K is the rate constant and initial concentration of the reactant is 0.5 M , then half-life is

For a reaction A+2B rarr C , the rate law is, rate= kxx[A]xx[B]^2 . If the rate constant of the reaction is 3.74xx10^(-2) M^(-2)s^(-1) , calculate the rate of the reaction when the concentrations of A and B are 0.126 M and 0.142 M respectively.

Half-life period for a first order reaction is 10 min. How much time is needed to change the concentration of the reactant from 0.08 M to 0.01 M ?

Conisder a reaction aG+bH rarr Products. When concentration of both the reactants G and H is doubled, the rate increases eight times. However, when the concentration of G is doubled, keeping the concentration of H fixed, the rate is doubled. The overall order of reaction is

For the reaction A + B rarr C , it is found that doubling the concentration of A increases the rate by 4 times, and doubling the concentration of B doubles the reaction rate. What is the overall order of the reaction ?