For a reaction scheme` A overset ( k _ 1 ) to B overset ( k _ 2 ) to C ` , if the rate of formation of B is set to be zero then the concentration of B is given by :

The rate law for a certain reaction is found to be : Rate = k[A] [B]^(2) How will the rate of this reaction compare if the concentration of A is doubled and the concentration of B is halved ? The rate will :

In a Radioactive decay A overset(k_1)toB overset(k_2)toC (K_1gtK_2) Initially B is not present, then correct curve for centration of B with respect to time is

In the sequence of reaction A overset(K_(1)) to B overset(K_(2))to C overset(K_( c)) to D, K_(3) gt K_(2) gt K_(1) then the rate determining step of the reaction is

A reaction is represented by : A to B slow and A+B to C (fast) where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of B will be given by :

A reaction is represented by A to^(k_1) B (slow). A+B to^(k_2) C (fast). Where k_1 and k_2 are the rate constants of the mechanistic steps. The rate of production of C will be given by