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प्रश्न
Answer the following in brief.
How will you determine activation energy graphically using the Arrhenius equation?
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उत्तर
Graphical representation of activation energy
Arrhenius equation is `"k" = "Ae"^((-"E"_"a")/("RT"))`
Taking the logarithm of both sides of Eqn. we obtain
In k = -`"E"_"a"/"RT" + "In A"`
Converting the natural base to base 10 we write
This equation is of the form of straight-line y = mx + c.
The Arrhenius plot of log10k versus `1/"T"` gives a straight line as shown in the diagram. A slope of the line is `-"E"_"a"/(2.303 "R")` with its intercept being log10A.
From a slope of the line, the activation energy can be determined.
Variation of log10k with 1/T
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संबंधित प्रश्न
The rate constant for the first-order reaction is given by log10 k = 14.34 – 1.25 × 104 T. Calculate activation energy of the reaction.
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