For a hypothetical reaction `A+B rarr C+D`, the rate `=k[A]^(-) ""^(1//2)[B]^(3//2)`. On doubling the concentration of A and B the rate will be

For a hypothetical reaction aA + bB rarr Product, the rate law is: rate = K[A]^(x)[B]^(y) , then

The rate law for a reaction between A and B is given by rate = k[A]^(n)[B]^(m) . On doubling the concentration of A and halving the concentration of B , the ratio of the new rate to the earlier rate of the reaction becomes

For a hypothetical reaction: A+B rarr Products, the rate law is r = k[A][B]^(0) . The order of reaction is

For a hypothetical reaction, A + B + C to Products, the rate law is determined to be rate = k[A][B]^(2) . If the concentration of B is doubled without changing the concentration of A and C, the reaction rate:

The rate expression for reaction A(g) +B(g) rarr C(g) is rate =k[A]^(1//2)[B]^(2) . What change in rate if initial concentration of A and B increases by factor 4 and 2 respectively ?