The time for half life period of a certain reaction A → products is 1 hour . When the initial concentration of the reactant ' A ', is 2.0 mol L^-1 , h - Chemistry MCQ AIEEE 2026 | ExamTest.live

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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?

Solution & Step-by-step Explanation

For a zero-order reaction: t_{1/2} = \frac{[ A ] _{0}}{2 k} Given [A]_{0} = 2.0 mol L^{- 1} and t_{1/2} = 1 h . 1 = \frac{2.0}{2 k} ⟹ k = 1 mol L^{- 1} h^{- 1} For a zero-order reaction, the time taken for concentration to change from C_{1} to C_{2} is: t = \frac{C _{1} - C _{2}}{k} Here, C_{1} = 0.50 mol L^{- 1} and C_{2} = 0.25 mol L^{- 1} . t = \frac{0.50 - 0.25}{1} = 0.25 h

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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?

4 h

0.5 h

0.25 h

1 h

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