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ChemistryChemical KineticsSecond & nth Order ReactionsMedium2 minPYQ_2021

ChemistryMediumsingle choice

For a reaction $A \to$ product, rate constant is $2 \times 1 0^{- 2} s^{- 1}$ . The initial concentration of $A$ is $1.0 mol dm^{- 3}$ . What is the value of $lo g \frac{1}{[ A ] _{t}}$ after 100 seconds?

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Answer:

Solution:

$k = 2 \times 1 0^{- 2} s^{- 1} (first order reaction) 2.303 lo g \frac{[ A ] _{0}}{[ A ] _{t}} = kt ([A]_{0} = 1 M) lo g \frac{1}{[ A ] _{t}} = \frac{k}{2.303} \times t = \frac{2 \times 1 0 ^{- 2} \times 100}{2.303} = 0.868$

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

⏱ 2mℹ️ Source: PYQ_2021

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