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.

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Solution

From Arrhenius equation, we obtain

Hence, the required energy of activation is 52.86 kJmol⁻¹.

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Similar questions

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

293 K

313 K

.Calculate the energy of activation?

Q. The rate of a reaction becomes four times when the temperature changes from

293 K

313 K

. Calculate the energy of activation

(E_{2})

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

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

Q. The rate of r

\times

n becomes

4

times when temp. changes from

293 K

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})

Q. The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is :
(Assume activation energy and pre-exponential factor are independent of temperature;

l n 2

=0.693; R = 8.314 J

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

)

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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.

From Arrhenius equation, we obtain Hence, the required energy of activation is 52.86 kJmol−1.

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.

From Arrhenius equation, we obtain

Hence, the required energy of activation is 52.86 kJmol⁻¹.