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Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsSecond & nth Order ReactionsEasy2 minPYQ_2021

ChemistryEasysingle choice

What is the half-life of a first order reaction if time required to decrease concentration of reactant from $1.0 M$ to $0.25 M$ is 10 hours?

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Answer:

Solution:

For first order reaction $k = \frac{1}{t} ln \frac{A _{0}}{At} = \frac{1}{10} \cdot ln \frac{1}{0.25} = \frac{ln 4}{10} h^{- 1}$ Half-life, $t_{1/2} = \frac{l n 2}{k} = \frac{l n 2}{l n 4/10} = \frac{10 \cdot l n 2}{2 \cdot l n 2}$ $t_{1/2} = 5 hour$

Stream:MHT_CETSubject:ChemistryTopic:Chemical KineticsSubtopic:Second & nth Order Reactions

⏱ 2mℹ️ Source: PYQ_2021

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