Problem: Food rots about 50 times more rapidly at 25 °C than when it is stored at 6 °C. Determine the overall activation energy for the processes responsible for its decomposition.A. 30 kJ/molB. 142 kJ/molC. -30 kJ/molD.  -142 kJ/molE. not enough information given

FREE Expert Solution

We’re being asked to determine the activation energy (Ea) for the process responsible when food rots about 50 times more rapidly at 25 °C than when it is stored at 6 °C. 


This means we need to use the two-point form of the Arrhenius Equation:


ln k2k1=-EaR[1T2-1T1]


where 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)


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Problem Details

Food rots about 50 times more rapidly at 25 °C than when it is stored at 6 °C. Determine the overall activation energy for the processes responsible for its decomposition.

A. 30 kJ/mol
B. 142 kJ/mol
C. -30 kJ/mol
D.  -142 kJ/mol
E. not enough information given

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