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

We’re being asked to determine the activation energy (E_a) 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:

$\boxed{\mathbf{ln}\mathbf{ }\frac{{\mathbf{k}}_{\mathbf{2}}}{{\mathbf{k}}_{\mathbf{1}}}\mathbf{=}\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}\mathbf{[}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\mathbf{]}}$

where k₁ = rate constant at T₁

k₂ = rate constant at T₂

E_a = activation energy (in J/mol)

R = gas constant (8.314 J/mol•K)

T₁ and T₂ = temperature (in K)