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The unit of rate constant for a zero order reaction is
A
$L^2\ mol^{-2}\ s^{-1}$
B
$s^{-1}$
C
$mol\ L^{-1}\ s^{-1}$
D
$L\ mol^{-1}\ s^{-1}$
Detailed Solution
For a zero order reaction: Rate = $k[\text{Reactant}]^0 = k$
So the rate constant has the same unit as the rate of reaction.
Rate = change in concentration / time = $\frac{mol\ L^{-1}}{s}$
Unit of k = $mol\ L^{-1}\ s^{-1}$
(General formula: unit of k = $(mol\ L^{-1})^{1-n}\ s^{-1}$; with n = 0 this gives $mol\ L^{-1}\ s^{-1}$.)
So the rate constant has the same unit as the rate of reaction.
Rate = change in concentration / time = $\frac{mol\ L^{-1}}{s}$
Unit of k = $mol\ L^{-1}\ s^{-1}$
(General formula: unit of k = $(mol\ L^{-1})^{1-n}\ s^{-1}$; with n = 0 this gives $mol\ L^{-1}\ s^{-1}$.)