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QJEEM06Chffe6: JEE Main 2006 Chemistry - Class 12 JEEM06Chffe6 Solution: Rate of a reaction can be expressed by Arrhenius equation as:…

Rate of a reaction can be expressed by Arrhenius equation as:
</mo></mrow><mi>k</mi><mo>=</mo><mi>A</mi><mstylescriptlevel="0"><mspacewidth="0.167em"></mspace></mstyle><mrowdata−mjx−texclass="ORD"><msup><mi>e</mi><mrowdata−mjx−texclass="ORD"><mo>−</mo><mi>E</mi><mrowdata−mjx−texclass="ORD"><mo>/</mo></mrow><mi>R</mi><mi>T</mi></mrow></msup></mrow></math></mjx−assistive−mml></mjx−container></mjx−assistive−mml></mjx−container></mo></mrow><mi>k</mi><mo>=</mo><mi>A</mi><mstyle scriptlevel="0"><mspace width="0.167em"></mspace></mstyle><mrow data-mjx-texclass="ORD"><msup><mi>e</mi><mrow data-mjx-texclass="ORD"><mo>−</mo><mi>E</mi><mrow data-mjx-texclass="ORD"><mo>/</mo></mrow><mi>R</mi><mi>T</mi></mrow></msup></mrow></math></mjx-assistive-mml></mjx-container></mjx-assistive-mml></mjx-container> In this equation, E represents

Multiple Choice Options

  • A the energy above which all the colliding molecules will react
  • B the energy below which colliding molecules will not react
  • C the total energy of the reacting molecules at a temperature, T
  • D the fraction of molecules with energy greater than the activation energy of the reaction

Step-by-Step Verified Solution

In Arrhenius equation K=Ae−E/RT,E is the energy of activation, which is required by the colliding molecules to react resulting in the formation of products.

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