For a chemical reaction rate law is, rate `= k{A]^(2)[B]`. If [A] is doubled at constant [B], the rate of reaction

Rate law for the reaction A + B to product is rate =K [A]^(2) [B]. What is the rate constant if the rate of the reaction at a given temperature is 0.22Ms^(-1) , when [A]=1 M and [B]=0.25 M?

For a chemical reaction mA→ xB The rate law is r = k [A]^(2) .If the concentration of A is doubled the reaction rate will be -

For a chemical reaction, mA to xB , the rate law is r=k[A]^2 . If the concentration of A is doubled, the reaction rate will be

For the reaction : 2A + 2B rarr 2C+ D , if concentration of A is doubled at constant [B], the rate increase by a factor of 4. If the concentration of B is doubled with [A] being constant the rate is double. Write the rate law of the reaction.

For a chemical reaction x A rarr y M the rate law is r=k[A]^3 . If the concentration of (A) is 'doubled the reaction rate will be

Rate law for the reaction A + B to product is rate= k[A]^2{B] . What is the rate constant, if rate of reaction at a given temperature is 0.22 Ms^-1, when [A] =1M and (B]= 0.25 M?

For the reaction A+BrarrC , the experimentally obtained rate law is ,rate k[A]^(2)[B] . What effect will produce on the rate reaction if the concentration of A is halved and that of B is doubled ?