🤓 Based on our data, we think this question is relevant for Professor Guloy's class at UH.

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**:

$\overline{){\mathbf{ln}}\left(\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}\right){\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}\frac{\mathbf{Ea}}{\mathbf{R}}\left[\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\right]}$

where:

**k _{1}** = rate constant at T

**k _{2}** = rate constant at T

**E _{a}** = activation energy (in J/mol)

**R** = gas constant (8.314 J/mol•K)

**T _{1} and T_{2}** = 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.