`aB+bBrarrP,dxx//dt=k[A]^(a)8[B]^(b)`. If conc. of A is doubled, rate is doubled. If B is doubled, rate becomes four times. Which is corect?

aA+bBrarr"Product",dx//dt=k[A]^(a)[B]^(b) . If conc. Of A is dounled, rate becomes four times. If conc. Of B is made four times, rate is doubled. What is the relation between rate of disappearance of A that B?

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 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 :

If each edge of a cube is doubled, then its volume: (a) is doubled (b) becomes 4 times (c) becomes 6 times (d) becomes 8 times

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

For a chemical reaction A+B rarr C it has been found that : (i) rate becomes double when the concentrations of A is doubled (ii) rate becomes 16 times when the concentrations of both A and B are doubled . The rate expression is :

In the reaction 2A+B to A_2B , Rate = k[A]^2 [ B ] if the concentration of A is doubled and that of B is halved, then the rate of reaction will:

In the reaction 2A+B to A_2B , Rate = k[A]^2 [ B ] if the concentration of A is doubled and that of B is halved, then the rate of reaction will: