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Chemical Kinetics question

2003 · Q102
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Chemical Kinetics question

2003 · Q102

NEETChemistryChemical KineticsMCQ+4 / −1
The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k=A⋅e−E∗/RTk = A \cdot {e^{ - E{}^ * /RT}}k=A⋅e−E∗/RT. Activation energy (E∗*∗) of the reaction can be calculated by plotting
  1. A
    k  vs  Tk\,\,vs\,\,TkvsT
  2. B
    k  vs  1log⁡Tk\,\,vs\,\,{1 \over {\log T}}kvslogT1​
  3. C
    log⁡ k  vs  1T\log \,k\,\,vs\,\,{1 \over T}logkvsT1​
  4. D
    log⁡ k  vs 1log⁡T\log \,k\,\,vs\,{1 \over {\log T}}logkvslogT1​
View written solutionFree

Correct answer: C

Arrhenius equation k = Ae−EaRTA{e^{ - {{{E_a}} \over {RT}}}}Ae−RTEa​​

⇒\Rightarrow⇒ log k = log A - Ea2.303RT{{{{E_a}} \over {2.303RT}}}2.303RTEa​​

Comparing it with equation of straight line i.e.,

y = mx + C

On plotting log k vs 1T{1 \over T}T1​, we get a straight line, the slope indicates the value of activation energy.

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