<u>Answer:</u> The correct statement about the complete combustion is 12 moles
<u>Explanation:</u>
We are given:
Moles of propane = 3.00 moles
To calculate the number of moles, we use the equation:
......(1)
For the given chemical equation:
![C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)](https://tex.z-dn.net/?f=C_3H_8%28g%29%2B5O_2%28g%29%5Crightarrow%203CO_2%28g%29%2B4H_2O%28g%29)
- <u>For carbon dioxide:</u>
By Stoichiometry of the reaction:
1 mole of propane produces 3 moles of carbon dioxide
So, 3.00 moles of propane will produce =
of carbon dioxide
Now, calculating the mass of carbon dioxide from equation 1, we get:
Molar mass of carbon dioxide = 44 g/mol
Moles of carbon dioxide = 9 moles
Putting values in equation 1, we get:
![9mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(9mol\times 44g/mol)=396g](https://tex.z-dn.net/?f=9mol%3D%5Cfrac%7B%5Ctext%7BMass%20of%20carbon%20dioxide%7D%7D%7B44g%2Fmol%7D%5C%5C%5C%5C%5Ctext%7BMass%20of%20carbon%20dioxide%7D%3D%289mol%5Ctimes%2044g%2Fmol%29%3D396g)
By Stoichiometry of the reaction:
1 mole of propane produces 4 moles of water
So, 3.00 moles of propane will produce =
of water
Now, calculating the mass of water from equation 1, we get:
Molar mass of water = 18 g/mol
Moles of water = 12 moles
Putting values in equation 1, we get:
![12mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(12mol\times 18g/mol)=216g](https://tex.z-dn.net/?f=12mol%3D%5Cfrac%7B%5Ctext%7BMass%20of%20water%7D%7D%7B18g%2Fmol%7D%5C%5C%5C%5C%5Ctext%7BMass%20of%20water%7D%3D%2812mol%5Ctimes%2018g%2Fmol%29%3D216g)
Hence, the correct statement about the complete combustion is 12 moles