For a hypothetical reaction `XrarrY`, the value of rate constant is `0.75sec^(-1)`. If the concentration of `X` is reduced to half, then value of the constant is

For a hypothetical reaction Ararr B , the rate constain is 0.25 s^(-1) . If the concentration of A is reduced to half, then the value of rate constant is

For a hypothetical reaction Ararr B , the rate constain is 0.25 s^(-1) . If the concentration of A is reduced to half, then the value of rate constant is

For a hypothetical reaction R rarr P the rate constant is 2944.06 s^(-1) if the concentration of R is reduced to half then the value of rate constant is

For a hypothetical reaction, ArarrP the rate constant is 0.12 s^(-1). which of the following relation is correct, if [R]_(0) is the initial concentration?

Consider the hypothetical reaction : A + 2B rarr C The rate remains constant when the concentration of A is doubled and the concentration of B is held concentration of B is doubled and the concentration of A is held constant. What are the orders of A and B in this reaction?

If the concentration units are reduced by n times, then the value of rate constant of first order will:

A reaction is of second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half ? What is the unit of rate constant of such a reaction ?

For a hypothetical reaction ArarrB , it is found that the rate constant = x s^(-1) . By what factor the rate is increased if the initial concentration of A is tripled?