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 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 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 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?

For a particular reaction (A rightarrow B) the rate constant is 0.693 (min)^-1 If the initial concentration of the reactant, A is 1 M, then the rate of reaction after 1 minute will be

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?

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?

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?

For a reaction A + B rarr product, the rate of the reaction was doubled when the concentration of A alone was reduced to half. Half life of reaction is doubled when concentration of B is reduced to half keeping concentration of A constant. Then order of reaction with respect to A and B are :