If `(dx)/(dt)=k[H_(3)O^(+)]n`
and rate becomes 100 times when pH changes from 2 to 1 Hence order of reactions is

If ((dx)/(dt))=k[H^(+)]^(n) and rate becomes 100 times when pH change from 2 to 1. Hence, order is :

If rate =k[H^(+)]^(n) and it becomes 100 times when the pH changes from 2 to 1, then the order of reaction is

The rate of a certain reaction is given by , rate =K [H^(+) ]^(n) . The rate increases 100 times when the pH changes from 3 to 1 . The order (n) of the reaction is ______.

For a reaction (d x)/(d t) = K[H^(+)]^(n) . If pH of reaction medium changes from two to one rate becomes 100 times of value at pH = 2 , The order of reaction is

The order of reaction is an experimentally determined quanity. It may be zero, poistive, negative, or fractional. The kinetic equation of nth order reaction is k xx t = (1)/((n-1))[(1)/((a-x)^(n-1)) - (1)/(a^(n-1))] …(i) Half life of nth order reaction depends on the initial concentration according to the following relation: t_(1//2) prop (1)/(a^(n-1)) ...(ii) The unit of the rate constant varies with the order but general relation for the unit of nth order reaction is Units of k = [(1)/(Conc)]^(n-1) xx "Time"^(-1) ...(iii) The differential rate law for nth order reaction may be given as: (dX)/(dt) = k[A]^(n) ...(iv) where A denotes the reactant. The rate constant for zero order reaction is where c_(0) and c_(t) are concentration of reactants at respective times.

The rate of a reaction becomes 4 times when temperature is raised from 293 K to 313 K. The activation energy for such reaction would be