How many moles of oxygen are required for the complete combustion of 2.2g of c3h8 to form carbon dioxide and water
C3H8 + 5O2 ==> 3CO2 + 4H2O
mols C3H8 = g/molar mass = = 2.2/44 = 0.05
Now use the coefficients in the balanced equation like this.
0.05 mols C3H8 x (5 mols O2/1 mol C3H8) = 0.05 x 5/1 = ?
To find out how many moles of oxygen are required for the complete combustion of C3H8, we first need to balance the chemical equation for the combustion reaction.
The combustion of C3H8 can be represented by the following balanced equation:
C3H8 + 5O2 → 3CO2 + 4H2O
From the balanced equation, we can see that 1 mole of C3H8 reacts with 5 moles of O2 to produce 3 moles of CO2 and 4 moles of H2O.
Now, let's calculate the moles of O2 required to react with 2.2g of C3H8:
1. Find the molar mass of C3H8 (propane):
C = 3 x 12.01 g/mol = 36.03 g/mol
H = 8 x 1.01 g/mol = 8.08 g/mol
Therefore, the molar mass of C3H8 is 36.03 g/mol + 8.08 g/mol = 44.11 g/mol.
2. Calculate the number of moles of C3H8:
Moles = Mass / Molar mass
Moles = 2.2 g / 44.11 g/mol ≈ 0.05 mol (rounded to two decimal places)
3. Determine the moles of O2 required:
From the balanced equation, we know that 1 mole of C3H8 reacts with 5 moles of O2.
Therefore, the moles of O2 will be 5 times the moles of C3H8.
Moles of O2 = 0.05 mol (C3H8) x 5 mol (O2)/1 mol (C3H8) = 0.25 mol O2
Therefore, 0.25 moles of oxygen are required for the complete combustion of 2.2g of C3H8 to form carbon dioxide and water.