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Arrhenius Equation

At 100 K, a...

Question

At $100 K$ , a reaction is $30$ % complete in $10$ minutes, while at $200 K$ , $30$ % is complete in $5$ minutes. The activation energy of the reaction is:

A

2050 J

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B

4000 J

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C

3000 J

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D

1150 J

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Solution

The correct option is D $1150 J$
We know,

${log}_{10} (\frac{k_{2}}{k_{1}}) = \frac{E_{a}}{2.303 R} \times (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$log 2 = \frac{E_{a}}{2.303 \times 8.314} \times (\frac{1}{100} - \frac{1}{200})$

$E_{a} = 1150 J$

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