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Arrhenius Equation

The rate of a...

Question

The rate of a particular reaction doubles when temperature changes from $27^{o} C$ to $37^{o} C$ . Calculate the energy of activation for such reaction. $[R = 8.314 J K^{- 1} m o l e]$

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Solution

$l o g \frac{K_{2}}{K_{1}} = \frac{E_{a}}{2.303 R} [\frac{1}{T_{1}} - \frac{1}{T_{2}}]$

$l o g \frac{2 K}{K} = \frac{E_{a}}{2.303 \times 8.314} \times [\frac{1}{300} - \frac{1}{310}]$

$\frac{0.3010 \times 2.303 \times 8.314 \times 300 \times 310}{10} = E_{a}$
$E_{a} = 53.603 K J / m o l$

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Q. The rate of a reaction doubles when its temperature changes from

300 K

310 K

. Activation energy of such a reaction will be:

(R = 8.314 J K^{- 1} {m o l}^{- 1} a n d log 2 = 0.301)

Q. The rate of a reaction triples when temperature changes from

20^{o} C

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. Calculate energy of activation for the reaction.

(R = 8.314 J K^{- 1} {m o l}^{- 1})

Q. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be:

(R = 8.314 J K^{- 1} m o l^{- 1}

l o g_{10} 2 = 0.301)

The rate of a particular reaction doubles when temperature change from

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Q. a) The rate of a particular reaction doubles when the temperature changes from 300 K to 310 K. Calculate the energy of activation of the reaction.
[Given :

R = 8.314 J K^{- 1} {m o l}^{- 1}

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b) Show that the half-life period of a first order reaction is independent of initial concentration of reacting species.

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