the combustion of propane produces carbon dioxide and steam C3H8(g)+5O2(g) 3CO2(g)+4H2O(g)
The combustion of propane produces carbon dioxide and steam C3H8(g)+5O2(g) 3CO2(g) +4H2O(g) all of the following statements concerning this reaction are correct except:
three molecule of carbon dioxide are formed per one molecule of propane consumed.
five molecules of oxygen are consumed per one molecule of propane consumed.
four moles of steam are formed per five moles of oxygen consumed.
the combined mass of reactants consumed equals the mass of products formed.
three grams of carbon dioxide are formed per five grams of oxygen consumed.
To balance the equation, we need to ensure that the number of atoms on both sides of the equation is the same.
The equation is already partially balanced, with the correct number of carbon (C) and hydrogen (H) atoms on both sides. However, the equation needs balancing for the oxygen (O) atoms.
Looking at the reactants, we have 5 oxygen molecules (O2), which means a total of 5 * 2 = 10 oxygen atoms.
Now looking at the products, we have 3 carbon dioxide molecules (CO2), which means a total of 3 * 2 = 6 oxygen atoms. Additionally, we have 4 water molecules (H2O), which means a total of 4 * 1 = 4 oxygen atoms.
In total, on the product side, we have 6 + 4 = 10 oxygen atoms, matching the number of oxygen atoms in the reactant.
So, the balanced equation is:
C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)
The balanced equation you provided represents the combustion of propane, which is a hydrocarbon compound. When propane (C3H8) is burned in the presence of oxygen (O2), it gets converted into carbon dioxide (CO2) and water vapor (H2O).
To understand how to balance this equation and determine the products of combustion, we follow a few steps:
Step 1: Count the number of atoms of each element on both sides of the equation.
On the reactant side (left side):
C: 3
H: 8
O: 10 (5 from O2)
On the product side (right side):
C: 3
H: 4 (2 from H2O)
O: 10 (6 from CO2, 4 from H2O)
Step 2: Balance the carbons by adjusting the coefficient of CO2.
Since there are 3 carbon atoms in propane (C3H8), we'll place a coefficient of 3 in front of CO2, making it 3CO2.
The balanced equation now becomes:
C3H8(g) + 5O2(g) -> 3CO2(g) + __H2O(g)
Step 3: Balance the hydrogens by adjusting the coefficient of H2O.
Propane has 8 hydrogen atoms (H), but the products currently provide only 4 hydrogen atoms. To balance the hydrogens, we'll place a coefficient of 4 in front of H2O.
The balanced equation now becomes:
C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(g)
Now the equation is balanced because both sides have an equal number of atoms for each element.
So, the combustion of propane (C3H8) produces 3 molecules of carbon dioxide (CO2) and 4 molecules of water vapor (H2O).