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Answer :
Final answer:
In complete and ideal combustion of gasoline using the principle of conservation of mass, the total combined mass of carbon dioxide and water produced when a gasoline tank holding 21 kg of gasoline burns consuming 84 kg of oxygen is 105 kg.
Explanation:
The subject of your question is based on the principle of conservation of mass, a fundamental concept in chemistry. The principle of conservation of mass states that the total mass of the reactants (the starting materials in a chemical reaction) is equal to the total mass of the products (the substances formed by the reaction). Hence, in the combustion (burning) of gasoline, the total combined mass of carbon dioxide and water that is produced would be equal to the sum of the masses of the gasoline and the oxygen consumed.
In your case, the total mass of gasoline and oxygen consumed is 21 kg (for gasoline) + 84 kg (for oxygen) = 105 kg. This means that given ideal condition and complete reaction, the total combined mass of carbon dioxide and water produced should be 105 kg.
Remember that this calculation assumes complete conversion of gasoline and oxygen into carbon dioxide and water, without production of other byproducts such as carbon monoxide and nitrogen oxides. Actual combustion processes may not be 100% efficient and may generate other byproducts.
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Rewritten by : Barada
21 kg + 85 kg = 106 kg
This is as straightforward as it gets. If however you need to determine how much of each product is produced, then the balanced equation is a must.
Usually, gasoline is expressed as octane in combustion reactions, which means that the balanced equation for its combustion is
2C8H18+25O2→16CO2+18H2O
But, like I've said, for the combined mass of the products all you really need to know is the combined mass of the reactants.
Addendum
Let's say you want to know exactly how much of each compound is formed. In this case, you must check for a limiting reagent. The number of moles of octane is
21⋅103
g⋅1 mole octane114.0 g=184.2
moles
The number of moles of oxygen is
85⋅103
g⋅1 mole O232.0 g=2656
moles
According to the mole ratio between these two, each 2 moles of octane need 25 moles of oxygen, so
noxygen that reacts=noctane⋅252=2303
moles
, which means that octane is the limiting reagent. The actual mass of oxygen that reacts is
2303 moles⋅32.0 g1 mole=73.7 kg
This means that the combined mass of the produced water and carbond dioxide is actually
21 kg+73.7 kg=94.7 kg
85 kg−73.7 kg=11.3 kg
of oxygen will not react. If you want to count this oxygen as well, the total combined mass of the products will again be 106 kg
.
