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