Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsFirst Order ReactionsMedium2 minQB

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The reaction, $X ⟶$ Product follows first order kinetics. In 40 minutes the concentration of X changes from 0.1 M to 0.025 M . Then the rate of reaction when concentration of X is 0.01 M.

Options:

Answer:

Solution:

$k = \frac{2.303}{40} lo g \frac{0.1}{0.025} = \frac{2.303}{40} lo g 4 = \frac{2.303}{40} \times 0.6021$

Now

$r a t e = k [X] = \frac{2.303}{40} \times 0.6021 \times 0.01 = 3.47 \times 1 0^{- 4} M min^{- 1}$

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:First Order Reactions

⏱ 2mℹ️ Source: QB

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