Half life of zero order reaction is 1 hour. If initial concentration of reactant is 2.0 mol L − 1 , find the time required to decrease concentration from 0.50 to 0.25 mol L − 1

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For a zero order reaction, the half-life is given by $t_{1/2} = \frac{[ A ] _{0}}{2 k}$

Substituting the given values:

$1 = \frac{2.0}{2 k} \Rightarrow k = 1.0 mol L^{- 1} hour^{- 1}$

The integrated rate equation for a zero order reaction is $[A]_{t} = [A]_{0} - k t$

For the concentration to decrease from $0.50 mol L^{- 1}$ to $0.25 mol L^{- 1}$ , the time required is:

$Δ t = \frac{[ A ] _{1} - [ A ] _{2}}{k}$

$Δ t = \frac{0.50 - 0.25}{1.0} = 0.25 hour$

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