The rate of hydrolosis of sucrose increases 4.1 times when the reaction temperature increases from 25°c to 35°c. Using this information (and appropriate assumptions) determine the energy of activation for the reaction. Please help?

1 Answer
Dave
Mar 8, 2018

3614 J/mole.....3.614 kJ/mole

Explanation:

You can use the straight line version of the Arrhenius Equation (the natural log version) to determine the energy of activation with these data. T1=298k, T2=308

#ln(k_1/k_2) = E_a/R(1/T_2-1/T_1)#

We'll assume that an increase in hydrolysis of sucrose of 4.1 times corresponds to k2/k1 = 4.1

#ln(1/4.1) = E_a/"8.314 J/molK""(1/308-1/298)#

Solve for Ea

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