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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.

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The rate constant is  0.049 s-1.

From the Arrhenius equation;

k = Ae^-Ea/RT

k = rate constant = ?

A =  frequency factor = 4.99×10^11 s−1

Ea = Activation energy = 86.4 kJ/mol or 86400 J

R = gas constant = 8.314 J/K/mol

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

k = 4.99 × 10^11e^- 86400/8.314 × 347

k = 0.049 s-1.

The rate constant is  0.049 s-1.

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