JEE Main 2017ChemistryChemical KineticsMediumMCQ

JEE Main 2017 — Chemical Kinetics Question with Solution

JEE Main 2017 (09 Apr Online)

Question

The rate of a reaction quadruples when the temperature changes from 300  to 310 K . The activation energy of this reaction is:

(Assume Activation energy and pre-exponential factor are independent of temperature; ln(2)=0.693; R=8.314 J mol-1K-1)

Choose an option

Show full solutionCorrect option: C
Correct answer
C107.2 kJmol-1

Step-by-step explanation

The activation energy, rate constant and temperature can be related using Arrhenius equation.

k=Ae-EaRT

lnk2k1=EaR 1T1-1T2 

ln4=EaR 1300-1310 

2×0.693=EaR 10300×310 

E a  =  2×0.693×300×310×8.314 10  = 107.2 kJ/mol

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About this question

This is a previous-year question from JEE Main 2017, 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.