What is enthelpy for combustion of glucose?

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SUMMARY

The enthalpy of combustion for glucose can be calculated using the enthalpies of formation for glucose (−1,268 kJ/mol), carbon dioxide (−393.5 kJ/mol), and water (−285.8 kJ/mol). The formula ∆H = Σ(∆Hf products) - Σ(∆Hf reactants) applies here, where Hess's law is crucial for determining the overall enthalpy change. This calculation is essential for understanding thermodynamic principles in chemistry and physics at a second-year level.

PREREQUISITES
  • Understanding of Hess's law
  • Knowledge of thermodynamic equations, specifically ∆H = U + PV
  • Familiarity with enthalpy of formation values
  • Basic principles of combustion reactions
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  • Research the application of Hess's law in thermodynamic calculations
  • Study the enthalpy of formation for various organic compounds
  • Learn how to perform combustion calculations in chemistry
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Chemistry students, particularly those in second-year physics or chemistry courses, and educators looking to clarify concepts related to thermodynamics and combustion reactions.

i_hate_math
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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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