Asked by Marcus
Many portable gas heaters and grills use propane, C3H8(g).
Using enthalpies of formation, calculate the quantity of heat produced when 15.0g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.
Using enthalpies of formation, calculate the quantity of heat produced when 15.0g of propane is completely combusted in air under standard conditions. Assume that liquid water is forming.
Answers
Answered by
DrBob222
C3H8 + 5O2 ==> 3CO2 +4H2O
mols Propane = grams/molar mass = estimated 0.34.
Convert mols propane to mols CO2 and mols H2O, then apply the following. You will need to look up the values for dH of CO2 and H2O(liquid) and C3H8. dH for O2 = 0
Post your work if you get stuck.
dHrxn = (n*dH products) - (n*dH reactants)
mols Propane = grams/molar mass = estimated 0.34.
Convert mols propane to mols CO2 and mols H2O, then apply the following. You will need to look up the values for dH of CO2 and H2O(liquid) and C3H8. dH for O2 = 0
Post your work if you get stuck.
dHrxn = (n*dH products) - (n*dH reactants)
Answered by
Jerald
-82 J
Answered by
Anonymous
56
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