Question

Consider the burning of LPG (propane C3H8)which produces carbon dioxide (CO2) and water vapor (H2O). The balanced chemical equation involving the reaction is C3H8+5O2= 3CO2+4H2O
Suppose 1.5 moles of C3H8 will be used, assume the following:
a. How many moles of O2 will be needed?
b. How many moles of H2O and CO2 will be formed?
c. How many grams will 1.5 moles C3H8 makes?
d. What volume (at STP)of O2 and CO2 are involved?
e. How many grams of water vapor will be formed?

Answer 1

C3H8 + 5O2 => 3CO2 + 4H2O
a. Use the coefficients in the balanced equation to convert anything to anything.
1.5 mols C3H8 x (5 mols O2/1 mol C3H8) = ?
b. same process.
c. grams = mols x molar mass but you didn't say grams of what.
d. Remember 1 mol of anything occupies 22.4 L at STP.
e. g H2O = mols H2O x molar mass H2O.

Answer 2

1.35g