[Algebrasucksbutilikeit]

I'm currently working on a Thermochemistry problem and i have no idea how to do this. I just learned it today :/

Using the information in the table to the right, calculate the enthalpy of combustion of each of the following substances:
Acetylene:    kJ/mol
Ethanol:      kJ/mol

Compound:           Enthalpy of formation:
methane(CH4)             -74.8
acetylene(C2H2)           226.77
ethanol(C2H6O)            -235.1
Carbon Dioxide(CO2)     -393.5
Water(H2o)                   -241.82

Please help me. I don't just want the answers, i want the work to go with it...any help given is much appreciated! Thank you

[AWK]

https://www.chemteam.info/Thermochem/HessLawIntro2.html

[Enthalpy]

If you learned it today, it must be in the lesson I guess.

Write a balanced chemical reaction, count the heats of formation of the reactants and products, deduce the heat of reaction.

Apparently, you can suppose that the combustion produces CO₂.

The heat of formation for water is indicated for vapour. Your computation will hence result in the "lower heating power".

Heats of formation given to 0.01kJ/mol are grotesque. I'd be very happy if they were known to 1kJ/mol.