[Stoves] H2O produce burning ethanol

[Kevin Chisholm]

Dear Crispin

The basic reaction is:

C2H5OH + 3 O2 ----> 2 CO2 + 3 H2O

Each mole of ethanol yields 3 moles of water

If you take the Heat of Reaction and subtract the enthalpy of the water 
vapor and the enthalpy of the CO2 at the temperature the gases leave the 
system, then the net result is the "net lower heating value" of ethanol.

(Obviously, you need to take into account to the heat absorbed by the 
Nitrogen in the air provided for combustion.)

Best wishes,

Kevin

Crispin Pemberton-Pigott wrote:
> Dear Friends
>
> How much H2O is produced burning 1 gram of ethanol?
>
> To calculate the LHV of ethanol I need to work out how much heat is lost not
> condensing the water produced during combustion.
>
> Secondly, who much heat is lost not cooling the other gases below 100 C?
>
> These together should be deducted from the HHV for the fuel to give a true
> LHV.
>
> Any ideas?
>
> Thanks
> Crispin
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