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We’re being asked to determine the activation energy of the rotting of food with a rate of 40 times (at 25°C) faster than 4°C.
This means we need to use the two-point form of the Arrhenius Equation:
k1 = rate constant at T1
k2 = rate constant at T2
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
Food rots about 40 times more rapidly at 25 °C than when it is stored at 4 °C. Determine the overall activation energy for the processes responsible for its decomposition.
a. 83.7 kJ/mol
b. 34.3 kJ/mol
c. 97.1 kJ/mol
d. 187 kJ/mol
e. 121 kJ/mol
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Based on our data, we think this problem is relevant for Professor Guloy's class at UH.