Asked by Jordin
The unbalanced equation for the combustion of ethanol is as follows:
C2H5OH(l) + O2(g) ¨ CO2(g) + H2O(g)
How much heat, in kJ, is liberated when 4.84 kg of C2H5OH(l) is burned?
Species Delta H‹f (kJ/mol)
H2O(g) -241.8
CO2(g) -393.5
C2H5OH(l) -277.7
Express the answer with three significant figures.
**I balanced the equation & got this:
C2H5OH(l) + 3O2(g) ¨ 2CO2(g) + 3H2O(g)
C2H5OH(l) + O2(g) ¨ CO2(g) + H2O(g)
How much heat, in kJ, is liberated when 4.84 kg of C2H5OH(l) is burned?
Species Delta H‹f (kJ/mol)
H2O(g) -241.8
CO2(g) -393.5
C2H5OH(l) -277.7
Express the answer with three significant figures.
**I balanced the equation & got this:
C2H5OH(l) + 3O2(g) ¨ 2CO2(g) + 3H2O(g)
Answers
Answered by
DrBob222
delta Hreaction = (n*deltaHProducts) - (n*delta H reactants)
Then delta Hrxn x (4.84/molar mass ethanol)
Then delta Hrxn x (4.84/molar mass ethanol)
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