# An #8.8*g# mass of propane is completely combusted. What mass of carbon dioxide will result?

##### 2 Answers

Approx.

#### Explanation:

WE have the stoichiometric equation:

Which tells us unequivocally that the combustion of 1 mole of propane gives 3 moles of carbon dioxide.

And then we simply access the molar quantity of propane:

And since, per the stoichiometric equation, if

At normal pressure and temperature,

24 litres at RTP (298K) or 22.4 litres at STP (273K)

#### Explanation:

1) The balanced equation gives us the mole ratio propane:oxygen which is 1:5 - this means that every mole of propane will require 5 moles of oxygen for complete combustion.

2) However we don't have one mole of propane, we have 8.8g which, using moles =mass/molar mass, equals 8.8/44 = 0.2 moles. (RMM of propane = 12x3 + 1x8 = 44, therefore molar mass = 44g/mol).

3) Applying the mole ratio, it follows that 0.2 moles of propane will react with 0.2x5 = 1 mole of oxygen.

4) One mole of any gas (assuming ideal behaviour, which is a perfectly reasonable assumption, especially with a gas like oxygen with small and non-polar molecules) occupies 24 litres at RTP and 22.4 at STP. Presto!