How much H2O and CO2 will be produced by burning 20L of propane?

Question

At STP (standard temperature & pressure), with full combustion, i.e. sufficient heat and oxygen available.

What's the calculation? 

________

Extra 

Any way I can find out how much the atmospheric CO2 concentration will rise in ppm, in a 500sqft room with 10 foot height (5000 cubic feet), where the normal CO2 level is ~400ppm ?

Thanks 

Update:

Update:

@billrussel42

1) "4•0.892 mol of H₂O"

>>>How much water produced in liters?

2) A) "3•0.892 mol of CO₂ is 2.676 mol"

>>>Why multiply 0.892 by 3?

Answer 1

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Propane + Oxygen ➜ Carbon Dioxide + water

C₃H₈ + 5O₂ ➜ 3CO₂ + 4H₂O

molecular weights

C = 12

H = 1

O = 16

C₃H₈ = 3•12+8 = 44

5O₂ = 10•16 = 160

3CO₂ = 3(12+32) = 132

4H₂O = 4•18 = 72

check 44 + 160 = 132 + 72 = 204

1 mole of C₃H₈ + 5 moles of O₂ ➜ 3 mole of CO₂ + 4 moles of H₂O

44 grams of C₃H₈ + 160 grams of O₂ ➜ 132 grams of CO₂ + 72 grams of H₂O

at STP (old def of STP, 1 atm) One mole of any ideal gas has a volume of 22.41L

20 L x 1 mol/22.41L = 0.892 mol

0.892 mol produces 3•0.892 mol of CO₂ and 4•0.892 mol of H₂O

5000 cubic feet = 141.6 m³

Density of Air 1.204 kg/m³ at 20ºC and 101.325kPa

141.6 m³ x 1.204 kg/m³ = 170 kg of air in the room

3•0.892 mol of CO₂ is 2.676 mol

CO₂ is 44 g/mol

44 g/mol x 2.676 mol = 118 g or 0.118 kg

0.118 / 170 = 0.00069 ratio

x 1000000 that is 690 PPM

add 400 to get 1090 PPM

note that there will probably be some CO mixed in with the CO₂