For a reaction rate `=K(A)^(1//2)(B)^(2)`. If concentration of A amd B are increased by factor of 4 and 2 respectively then rate is changed by the fraction :-

For A_((s))+B_((s))toC_((s)) ,rate= k[A]^(1//2)[B]^(2) , if initial concentration of A and B are increased by factors 4 and 2 respectively, then the initial rate is changed by the factor:

For A_((s))+B_((s))toC_((s)) ,rate= k[A]^(1//2)[B]^(2) , if initial concentration of A and B are increased by factors 4 and 2 respectively, then the initial rate is changed by the factor:

For A_((s))+B_((s))toC_((s)) ,rate= k[A]^(1//2)[B]^(2) , if initial concentration of A and B are increased by factors 4 and 2 respectively, then the initial rate is changed by the factor:

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 ?

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 ?

Consider the reaction 2A+B rarr C+D. If the rate expression is rate= K [A]^2 [B]^1 and if concentration of the reactants are increased by three times, the rate of the reaction will increase by:

The reaction A+B to products is first order in each of the reactants. (a) How does the rate of reaction change if the concentration of A is increased by factor 3 ? (b) What is the change in the rate of reaction if the concentration of A is halved and concentration of B is doubled ?

The experimental rate law for a reaction 2A + 2B rarr Product, is V prop C_(A) C_(B)^(1//2) . If the concentration of both A and B are doubled the rate of reaction increases by a factor of