What is enthelpy for combustion of glucose?

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To calculate the enthalpy for the combustion of 1 mole of glucose, the enthalpy of formation values for glucose, carbon dioxide, and water are essential. The combustion reaction can be analyzed using Hess's law, which states that the total enthalpy change is the sum of the enthalpy changes for individual steps. The relevant enthalpy values are ∆(Glucose) = −1,268 kJ/mol, ∆(Carbon Dioxide) = −393.5 kJ/mol, and ∆(Water) = −285.8 kJ/mol. Understanding these concepts is crucial for solving thermodynamic problems related to combustion. The discussion emphasizes the need for a structured approach to homework problems in chemistry.
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The enthalpies of formation with reference to (2) are: ∆(Glucose)= −1,268 /, ∆(Carbon Dioxide)= −393.5 ./, ∆(water)= −285.8 /.

How do I calculate the enthalpy for the combustion of 1 mole of glucose?

I know H = U + PV and ∆H = Q + Wother, but I am confused by all the chemistry involved!
 
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Have you heard of Hess's law?
 
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No I haven't. This was a question in a past exam that I'm stuck on, it could be unrelated. Was I right to consider it as a purely thermodynamic (2nd year physics level) problem?
 
This should be posted in a homework forum with an attempt at a solution.

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