Question

Consider the Combustion of Propane (C3H8)by O2 and H2o.

                             C3H8 +5O2 --> 3Co2+ 4H2o

D)    At standard temperature and pressure, what volume of oxygen would be required to burn 100 g of propane? If air is 21 percent oxygen, what volume of air at STP would be required?

E) At standard temperature and pressure, what volume of Co2 would be produced when 100g of propane are burned?

Answer 1

Molar mass of Propane = 12 * 3 + 8 * 1 = 44 gm/mol

Number of moles of Propane = 100/44 = 2.27 moles

Moles of O2 required = 5 * number of moles of propane = 500/44 moles = 11.36 moles

air contains 21% oxygen

Moles of air required = 11.36 * 100/21 = 54.095 moles

at STP, 1 mole contains 22.4 L

Volume of air required = 54.095 * 22.4 = 1211.73 L

E)

Moles of CO2 produced = 300/44 = 6.818 moles

at STP, 1 mole contains 22.4L

Volume of CO2 produced = 6.818 * 22.4 = 152.72 L