The rate of r $\times$ n becomes $4$ times when temp. changes from $293 K$ to $313 K$ Calculate energy of activation (Ea) of the rxn assuming that it does not change with temp. $(R = 8.3 / 4 J K^{-} m o l^{- 1})$

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Solution

$l o g \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{2.303 \times R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$l o g (4) = \frac{E_{a}}{2.303 \times 8.314} (\frac{1}{293} - \frac{1}{313})$

$E_{a} = 52.85 K J {m o l}^{- 1}$

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Q. The rate of a reaction becomes four times when the temperature changes from 293K to 313 K. Calculate the energy of activation

(E_{a})

of the reaction assuming that it does not change with temperature.

[R = 8.314 J K^{- 1} m o l^{- 1}, l o g 4 = 0.6021]

The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.

Q. The rate of the reaction quadruples when the temperature changes from

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Q. Calculate the activation energy for a reaction of which rate constants becomes 4 times when temperature changes from

30^{0} C

50^{0} C

[R= 8.314

J m o l^{- 1} K^{- 1}

]

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

20^{o} C

50^{o} C

. Calculate energy of activation for the reaction.

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

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The rate of r×n becomes 4 times when temp. changes from 293K to 313K Calculate energy of activation (Ea) of the rxn assuming that it does not change with temp. (R=8.3/4JK−mol−1)

logk2k1 = Ea2.303×R(1T1−1T2)log(4)=Ea2.303×8.314(1293−1313)Ea=52.85 KJ mol−1

The rate of r $\times$ n becomes $4$ times when temp. changes from $293 K$ to $313 K$ Calculate energy of activation (Ea) of the rxn assuming that it does not change with temp. $(R = 8.3 / 4 J K^{-} m o l^{- 1})$

$l o g \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{2.303 \times R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$l o g (4) = \frac{E_{a}}{2.303 \times 8.314} (\frac{1}{293} - \frac{1}{313})$

$E_{a} = 52.85 K J {m o l}^{- 1}$