Answer: 163.6g H2O
Step-by-step explanation:
The balanced chemical equation for the combustion of propane is:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
This means 1 molecule of C3H8 react with 5 molecules of O2 to produce 3 molecules of CO2 and 4 molecules of H2O.
Molar mass C3H8 = 44 g/mol
According to the stochiometric coefficients 1 mol C3H8 will form 4H2O
100g C3H8 to mol = 100 g / 44 g/mol = 2.273 mol
This will produce 2.273*4 H2O = 9.09 mol H2O
Molar mass H2O = 18 g/mol
Mass of 9.09 mol H2O = 9.09 mol * 18 g/mol = 163.6 g H2O
Therefore, 163.6g of H2O will be formed from the combustion of 100g of C3H8