Consider the following statements which is/are incorrect :

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Rate constant K is equal to collision frequency ‘A’ if $E_{a} = 0$

Rate constant K is equal to collision frequency ‘A' if $E_{a} = α$

Increase in concentration of reactant increases the rate of a zero order reaction

$Log e^{k} vs \frac{1}{T}$ is a straight line

answer is A, C, D.

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Detailed Solution

A) The rates of zero order reactions do not vary with increasing or decreasing reactants concentrations B&C) According to Arrhenius equation, $K = A . e^{- Ea / RT} if E_{a} = 0 and then k = A .$ So statement C is incorrect D) The Arrhenius plot is obtained by plotting the logarithm of the rate constant (k) versus the inverse temperature (1/ T) , results a negative sloped line.