First you need to write a balanced equation. You are given that propane undergoes a combustion reaction that produces carbon dioxide and water.
Unbalanced: C3H8 + O2 ---> CO2 + H2O
Balanced: C3H8 + 5O2 ---> 3CO2 + 4H2O
Givens:
42.0 grams C3H8 (Molecular mass 44.0 g)
115.0 grams O2 (Molecular mass 32.0 g)
Molecular mass of CO2: 44.0 g
Mole ratio 1:5:3:4 (C3H8:O2:CO2:H2O)
Then you need to find which of the reactants are the limiting reactant (lowest value) and which is the excess reactant. The limiting reactant is what you will base the rest of the problem on. To do this, you convert each measurement to moles from grams.42.0 g C3H8 / (44.0 g) = .955 moles C3H8 115.0 g
To determine the grams of carbon dioxide produced, we first balance the chemical equation for the combustion of propane: C3H8 + 5O2 -> 3CO2 + 4H2O. Using the stoichiometry of the balanced equation, we find that 42 grams of propane will produce 3 * (44 g/mol) = 132 grams of carbon dioxide. For the water produced, 42 grams of propane will produce 4 * (18 g/mol) = 72 grams of water.
First you need to write a balanced equation. You are given that propane undergoes a combustion reaction that produces carbon dioxide and water.
Unbalanced: C3H8 + O2 ---> CO2 + H2O
Balanced: C3H8 + 5O2 ---> 3CO2 + 4H2O
Givens:
42.0 grams C3H8 (Molecular mass 44.0 g)
115.0 grams O2 (Molecular mass 32.0 g)
Molecular mass of CO2: 44.0 g
Mole ratio 1:5:3:4 (C3H8:O2:CO2:H2O)
Then you need to find which of the reactants are the limiting reactant (lowest value) and which is the excess reactant. The limiting reactant is what you will base the rest of the problem on. To do this, you convert each measurement to moles from grams.42.0 g C3H8 / (44.0 g) = .955 moles C3H8 115.0 g× (5 moles) / (32.0 g) = 18.0 moles O2 Because propane is the limiting reactant (less of it than oxygen), the amount of water produced can only be as much as the propane. Take the amount of propane and use stoichiometry to find the amount of water produced in grams.
42.0 g C3H8 / (44.0 g) × (4 moles) × (18 g) = 68.7 grams H2O
In the presence of excess oxygen, propane burns to form water and carbon dioxide. When not enough oxygen is present for complete combustion, incomplete combustion occurs when propane burns and forms water, carbon monoxide, and carbon dioxide.
When methane is burned in oxygen, assuming complete combustion, the products are carbon dioxide and water.
Carbon dioxide (CO2) is a product of the combustion of propane.
The products of the complete combustion of propane are carbon dioxide (CO2) and water vapor (H2O). This reaction releases heat energy and is used in many heating and cooking applications.
When propane is combined with oxygen and ignited, it undergoes combustion to produce carbon dioxide, water vapor, and heat. This reaction releases energy that can be used for heating or cooking purposes.
30 moles
In the presence of excess oxygen, propane burns to form water and carbon dioxide. When not enough oxygen is present for complete combustion, incomplete combustion occurs when propane burns and forms water, carbon monoxide, and carbon dioxide.
When propane is combined with oxygen and ignited, it undergoes combustion to produce carbon dioxide, water vapor, and heat. This reaction releases energy that can be used for heating or cooking purposes.
The products of the complete combustion of propane are carbon dioxide (CO2) and water vapor (H2O). This reaction releases heat energy and is used in many heating and cooking applications.
37.8
When methane is burned in oxygen, assuming complete combustion, the products are carbon dioxide and water.
Carbon is burned to carbon dioxide, a colorless gas.
11.0g
Oxygen Nitrogen Argon Carbon Dioxide Propane Helium Hydrogen Acetylene
Burning propane is called combustion, in which propane combines with oxygen to form carbon dioxide and water.
When hydrocarbons are burned, carbon dioxide is formed. If the hydrocarbon is burned in low amount of oxygen, carbon monoxide can be formed. Carbon monoxide is harmful for animals.
Yes, indeed, as anyone with a propane-fueled heater can experience!