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Klio2033 [76]
3 years ago
8

Calculate the rate constant, , for a reaction at 74.0 °C that has an activation energy of 86.4 kJ/mol and a frequency factor of

4.99×1011 s−1.
Chemistry
1 answer:
Lelechka [254]3 years ago
5 0

The rate constant is 4.84 * 10^11 s-1.

From the Arrhenius equation;

k = Ae^-Ea/RT

k = rate constant = ?

A =  frequency factor = 4.99×1011 s−1

Ea = Activation energy = 86.4 kJ/mol

R = gas constant = 8.314 J/K/mol

T = Absolute temperature = 74.0 °C + 273 = 347 K

k = 4.99×10^11e^- 86.4/8.314 * 347

k = 4.84 * 10^11 s-1.

The rate constant is 4.84 * 10^11 s-1.

Learn more: brainly.com/question/626780

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