Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: dyeownsme on December 06, 2004, 02:26:41 PM
-
Ethanol burns in air according to this equation:
C2H5OH (L) + O2 (G) -----> CO2 (G) + H20 (L)
And asks calculate the mass of ethanol needed to produce 8.00L of CO2 (g) at 27 degrees C at 1.00 atm
I figured the mass produced but am not sure of method to solve this equation.
I am also confused about finding the Delta H for a reaction with on the formula given... it is an reaction bettween NaOH adn HCl very basic but im stumped....
Thanks for any help whatsoever
-
convert 8L of CO2 into number of moles
find the required number of moles of ethanol, then convert to mass.
delta H is amount of energy evolved per mole of limiting reagent.
delta H for neutralisation is change in enthalpy during neutralisation per mole of water formed.
-
There is also a small error in the equation you were given. Due to the heat of combustion, any water that is formed will be formed as a gas and not as a liquid. This may have an effect on the calculation since the presence of the gaseous water will alter the overall pressure. So I would make sure that you should be disregarding water before finishing the problem.