If 2.33L of propane (C3H8) at 24.0C and 67200 Pascals is completely burned with excess oxygen, how many moles of carbon dioxide gas will be produced?

0.182 moles of CO₂ are produced by this combustion

Explanation:

First of all, we state the combustion reaction:

C₃H₈  +  5O₂  → 3CO₂  +  4H₂O

As we do not have data from the oxygen, we assume it as the excess reactant. Let's determine the moles of propane, by the Ideal Gases Law.

We convert pressure from Pa to atm

67200 Pa . 1 atm /101300 Pa = 0.663 atm

P . V = n . R . T

0.633 atm . 2.33L = n . 0.082 . 297K

(0.633 atm . 2.33L) / (0.082 . 297K) = n

n = 0.0606  moles

Now we analyse the stoichiometry. Ratio is 1:3.

1 mol of propane can produce 3 moles of carbon dioxide

Then, 0.0606 moles of propane may produce (0.0606 . 3) /1 = 0.182 moles

In conclussion, 0.182 moles of CO₂ are produced by this combustion

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.