# Thermodynamics of Reactions with Glucose

## Homework Equations

ΔH rxn = ΔH products - ΔH reactants
ΔU = q + w

## The Attempt at a Solution

Pretty overwhelmed with the entire problem. Since the ΔH's of all reactants and products were in the literature for the reference temperature of 298.15 K, I was able to plug them in and get the value for that temperature. I am not sure how it changes with temperature increase?

Can anyone point me in the right direction?

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chemisttree
Homework Helper
Gold Member
Perhaps heat capacity(-ies) is the reason where delta T = 298.15 K - 330.15 K.

Ah, okay I was able to the the change in enthalpy for 330.15 K by Hess's law, and adding delta H rxn (298.15K) to the integral of delta Cp dT integrated from To to T.

Now I'm stuck on b. part ii. I can't find any examples anywhere on calculating problems like this and my professor is so highly educated (MIT, Harvard, UPenn) that I can't understand him.

Ahh, any help is appreciated!

chemisttree