Problem: 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/molb. 34.3 kJ/molc. 97.1 kJ/mold. 187 kJ/mole. 121 kJ/mol

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FREE Expert Solution

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:


lnk2k1 = -EaR1T2-1T1


where:

k1 = rate constant at T1 

k2 = rate constant at T

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 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.