In the reaction `aA+bB to` products, if concentration of A is doubled (keeping B constant) the initial rate becomes four times and if B is doubled (keeping A constant), the rate becomes double. What is the rate law equation and order of reaction ?

In the reaction "a A"+"b B"to Products, if only concentration of A is doubled the rate becomes quadrupled and if further the vessel is reduced to half the volume, the rate becomes 8 times. The overall order of reaction is

In the reaction A + B rarr Products, keeping [A] constant if [B] is doubled , the rate becomes double and keeping [B] constant if [A] is doubled , the rate becomes four times. The order of reaction is :

In a reaction A + B to Products (i) If the initial concentration of A is doubled and B is kept constant, the rate of the reaction is doubled (ii) If the initial concentration both A and B are doubled the rate of reaction becomes eight times The rate law of the reaction is :

For a zero order reaction, The rate becomes double when the order of the reaction.

For a 1st order reaction if concentration is doubled then rate of reaction becomes