For a reaction `A \rightarrow B`, K is `1xx10^(-2)Lmol^(-1)sec^(-1)` .If conc of A is 2.0`molL^(-1)` ,the rate of reaction would be

The rate constant for the reaction A rarr B is 2xx10^(-4)"L mol"^(-1)"min"^(-1) . The concentration of A at which rate of the reaction is ((1)/(20))xx10^(-5)"M sec"^(-1) is :

For the reaction 2NOBr to 2NO_2 + Br_2, the rate law is rate = k[NOBr]^2 . If the rate of a reaction is 6.5xx10^(-6) molL^(-1)s^(-1) , when the concentration of NOBr is 2xx10^(-3) molL^(-1) .What would be the rate constant of the reaction?

The rate constant for the reaction A rarr B is 2 xx 10^(-4) mol^(-1) . The concentration of A at which rate of the reaction is (1//2) xx 10^(-5) M sec^(-1) is -

For a reaction 2A rightarrow B ,when concentration of reactant is 0.2molL^(-1) ,rate of disapperance of "A" is found to be 2times10^(-4)molL^(-1)s^(-1) .If pressure is increased 2 times then rate of reaction increases four times.Calculate rate constant of reaction.

For the reaction A+B to product [A]=[B]=1 M the rate of reaction is 2xx10^(-2 ) mol dm^(-3) sec^(-1) , then the rate of reaction at the time of 90 % of each of the reactants are converted into product is

The rate constant of a reaction at 300 K is 1.6 xx 10^(-3) sec^(-1) and at 310K it is 3.2 xx 10^(-3) sec^(-1) the activation energy of the reaction approximately in kcals is

The specific rate constant for a first order reaction is 1 times 10^–3 sec^–1 . If the initial concentration of the reactant is 0.1 mole/lt, the rate of reaction mol l^–1 sec^–1 is:

In the reaction A+2B to 3C + 2D , the rate of disappearance of B is 1 xx 10^(-2) mol L^(-1)s^(-1) . What will be the rate of the reaction and rate of change in concentration of A and C?