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The time for half life period of a certain reaction $A \to$ Products is 1 hour. When the initial concentration of the reactant ‘A’. is 2.0 ${mol L}^{- 1}$ , how much time does it take for its concentration to come from 0.50 to 0.25 ${mol L}^{- 1}$ if it is a zero order reaction?

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0.25 h

4 h

0.5 h

answer is C.

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Detailed Solution

For the reaction $A \to$ Product given $t_{1/2} = 1 hour$ for a zero order reaction $t_{1/2} = \frac{[A_{0}]}{2k}$ $or k = \frac{[A_{0}]}{{2t}_{1/2}} = \frac{2}{2 × 1} {= 1 mol lit}^{-1} {hr}^{-1}$ Further for a zero order reaction

$k = \frac{dx}{dt} = \frac{change in concetration}{time}$

$1 = \frac{0.50 - 0.25}{time}$

$∴ time = 0.25 hr.$

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