For `2A+B+Cto` Products, rate law is given by rate `=" k [A] [B]"^(2)` & rate constant (k) is `2xx10^(-6)M^(-2)-s^(-1)`. Then rate of the reaction become `2xx10^(-9)"M - s"^(-1)` only when [A] , [B] , [C] are respectively

The rate constant of a reaction is 1.2xx10^(-5)mol ^(-2)"litre"^(2) S^(-1) the order of the reaction is

If the rate of reaction between A and B is given by rate =k[A][B]^(2) , then the reaction is :

If in a chemical reaction, A+B to Products, the rate law is given the expression : rate = k[A](1/2)[B]^(3/2) . What is the order of the reaction?

For a reaction, A+B to Products, the rate law is given by: r=k[A]^(1//2)[B]^(2) . What is the order of 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 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?