The standard enthalpy of formation of glucose is -1273.3kJ/mol, and for carbon dioxide it is -393.5kJ/mol, and for water -285.8 kJ/mol. What is the standard enthalpy of combustion of glucose, C6H12O6?

The reaction equation has the form C6H12O6 + xO2 -> yCO2 + zH2O. Balancing carbons, y=6. Balancing hydrogens, z=6, so by balancing oxygen atoms, x=6. Then we use a Hess's law cycle (to be shown during interview) to find that the enthalpy of combustion is -(-1273.3kJ/mol)+(-6x-393.5kJ/mol+-6x-285.8kJ/mol) = -2802.5kJ/mol.

Answered by Amber C. Chemistry tutor

31753 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What factors affect acidity in solution?


Please give the definition of Le Chatilier's principle. Use this to explain what would happen if you increased the temperature of an equilibrium in which the forwards reaction is exothermic.


Why does phenol react more readily with bromine than benzene?


How does ionisation energy change down a group?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences