For a first order reaction, intercept of the graph between lo g ( [ A ] t [ A ] 0 Y -axis) and time. (X-axis) is equal to

For 1 st order reaction, 2.303 lo g [ A ] t [ A ] 0 = kt lo g [ A ] t [ A ] 0 = 2.303 k ⋅ t , y = mx ; C = 0 [ Intercept = 0 ]

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Chemistry - Chemical Kinetics Question with Solution | TestHub

ChemistryChemical KineticsSecond & nth Order ReactionsEasy2 minPYQ_2021

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For a first order reaction, intercept of the graph between $lo g (\frac{[ A ] _{0}}{[ A ] _{t}} Y$ -axis) and time. (X-axis) is equal to

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Solution:

For $1^{st}$ order reaction, $2.303 lo g \frac{[ A ] _{0}}{[ A ] _{t}} = kt$ $lo g \frac{[ A ] _{0}}{[ A ] _{t}} = \frac{k}{2.303} \cdot t, y = mx; C = 0 [Intercept = 0]$

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

⏱ 2mℹ️ Source: PYQ_2021

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