The combustion of propane may be described by the chemical equation
C3H8(g)+5O2(g)⟶3CO2(g)+4H2O(g)
How many grams of O2(g) are needed to completely burn 61.9 g C3H8(g)?
To determine the amount of O2(g) required to completely burn 61.9 g of C3H8(g), we need to use the stoichiometry coefficients from the balanced chemical equation.
In the given equation: C3H8(g) + 5O2(g) ⟶ 3CO2(g) + 4H2O(g)
The stoichiometry coefficients indicate that 1 mole of C3H8 requires 5 moles of O2. To find the amount of O2 needed, we need to convert grams of C3H8 to moles using its molar mass and then use the stoichiometry ratios.
Molar mass of C3H8:
C = 12.01 g/mol x 3 = 36.03 g/mol
H = 1.01 g/mol x 8 = 8.08 g/mol
Total molar mass = 36.03 g/mol + 8.08 g/mol = 44.11 g/mol
Moles of C3H8 = mass / molar mass = 61.9 g / 44.11 g/mol = 1.404 mol
According to the stoichiometry, 1 mole of C3H8 requires 5 moles of O2. Therefore,
Moles of O2 = 1.404 mol x 5 = 7.02 mol
Now we need to convert moles of O2 to grams using its molar mass.
Molar mass of O2: O = 16.00 g/mol x 2 = 32.00 g/mol
Grams of O2 = moles x molar mass = 7.02 mol x 32.00 g/mol = 224.64 g
Therefore, 224.64 grams of O2(g) are needed to completely burn 61.9 g of C3H8(g).
To determine the grams of O2 required to completely burn 61.9 g of C3H8, we need to use the stoichiometry of the chemical equation.
The balanced equation tells us that for every 1 mole of C3H8, we need 5 moles of O2. We can calculate the molar mass of C3H8 to convert grams to moles.
Molar mass of C3H8:
C3H8 = (3 * molar mass of Carbon) + (8 * molar mass of Hydrogen)
First, let's find the molar mass of Carbon (C):
Molar mass of Carbon = 12.01 g/mol
Next, let's find the molar mass of Hydrogen (H):
Molar mass of Hydrogen = 1.01 g/mol
Now we can calculate the molar mass of C3H8:
Molar mass of C3H8 = (3 * 12.01 g/mol) + (8 * 1.01 g/mol)
Using these values, calculate the molar mass of C3H8.
Once we have the molar mass of C3H8, we can convert the given 61.9 g of C3H8 to moles by using the equation:
Number of moles = Given mass / Molar mass
Now we have the number of moles of C3H8. Since the stoichiometric ratio states that 1 mole of C3H8 reacts with 5 moles of O2, we can use this ratio to find the number of moles of O2 required.
Finally, to find the grams of O2 required, we can use the equation:
Mass = Number of moles * Molar mass
By following these steps, we can determine the grams of O2 required to completely burn 61.9 g of C3H8.
C3H8(g) + 5O2(g)⟶3CO2(g) + 4H2O(g)
mols C3H8 = grams/molar mass = 61.9/44 = estimated 1.3 but notice that's just an estimate.
Every mole C3H8 requires 5 mols O2; therefore, mols O2 needed = estimated 5*1.3 = 6.5
Grams O2 = mols x molar mass = approx 6.5 x 32 = ?
Post your work if you get stuck.