The half-life for a zero order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in $mol L^{- 1} s^{- 1}$ ) for the reaction is

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$2.0 \times 10^{- 4}$

$1.0 \times 10^{- 2}$

$2.0 \times 10^{- 3}$

$1.0 \times 10^{- 4}$

answer is B.

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Detailed Solution

For zero order reaction

$\begin{array}{l} t_{1 / 2} = \frac{a}{2 k} \Rightarrow k = \frac{a}{2 t_{1 / 2}} \\ k = \frac{0 .02}{2 \times 100} = 1 .0 \times 10^{- 4} {molL}^{- 1} s^{- 1} \end{array}$

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