Question

specific reaction rate of reaction quadruples when temperature changes from 30°c to 50°c calculate energy of activation​

Answer 1

Answer:

From Arrhenius equation, we obtain

Hence, the required energy of activation is 52.86 kJ mol - 1.

Answer 2

The activation energy for the reaction is 56217.3 J/mol

Explanation:

According to the Arrhenius equation,

$K=A\times e^{\frac{-Ea}{RT}}$

or,

$\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$K_1$ = rate constant at $30^oC$ = x

$K_2$ = rate constant at $50^oC$ = 4x

$Ea$ = activation energy for the reaction = ?

R = gas constant = 8.314 J/mole.K

$T_1$ = initial temperature = $30^oC=273+30=303K$

$T_2$ = final temperature = $50^oC=273+50=323K$

Now put all the given values in this formula, we get

$\log (\frac{4x}{x})=\frac{Ea}{2.303\times 8.314J/mole.K}[\frac{1}{303K}-\frac{1}{323K}]$

$0.60=\frac{Ea}{2.303\times 8.314J/mole.K}[\frac{1}{303K}-\frac{1}{323K}]$

$E_a=56217.3J/mol$

Therefore, the activation energy for the reaction is 56217.3 J/mol

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