JEE Main 2016ChemistryChemical KineticsMediumMCQ

JEE Main 2016 — Chemical Kinetics Question with Solution

JEE Main 2016 (03 Apr)

Question

Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H 2 O 2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M , the rate of formation of O2 will be:

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Show full solutionCorrect option: D
Correct answer
D6.93×10-4 mol min-1

Step-by-step explanation

H 2 O 2 → H 2 O+ 1 2 O 2

-d[H2O2]dt=d[H2O]dt=2d[O2]dt



t12=25

t 1 2 = 0.69314 k

k =  0.69314 25

rate of reaction = k[H2O2]

∴ d[O2]dt=12×k[H2O2]

=12×0.6931425×0.05

=6.93×10-4 mol min-1

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About this question

This is a previous-year question from JEE Main 2016, covering the Chemical Kinetics chapter of Chemistry. PrepSharp catalogues every PYQ from JEE Main with a verified answer key and step-by-step solution prepared by IIT alumni — so you can search by chapter, topic or year and revise efficiently.