How many grams of carbon dioxide gas are formed when 11.9g of liquid hexane (C6H14) is combusted?
2C6H14 + 19O2 ==> 12CO2 + 14H2O
mols hexane = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Hexane to mols CO2. You can see that 2 mols hexne will produce 12 molsl CO2.
Convert mols CO2 to grams. grams = mols x molar mass
To find the number of grams of carbon dioxide gas formed when 11.9g of liquid hexane (C6H14) is combusted, we need to use the balanced chemical equation for the combustion of hexane.
The balanced equation is:
C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O
From the balanced equation, we can see that 1 mole of hexane (C6H14) reacts with 19/2 moles of oxygen gas (O2) to produce 6 moles of carbon dioxide gas (CO2).
First, we need to find the moles of hexane present in 11.9g. To do this, we use the molar mass of hexane, which is 86.18 g/mol.
Moles of hexane (C6H14) = Mass / Molar mass
Moles of hexane = 11.9g / 86.18 g/mol ≈ 0.138 moles
Now that we have the moles of hexane, we can use the mole ratio from the balanced equation to find the moles of carbon dioxide formed.
Moles of carbon dioxide (CO2) = Moles of hexane (C6H14) × (6 moles CO2 / 1 mole C6H14)
Moles of carbon dioxide = 0.138 moles × (6/1) ≈ 0.828 moles
Finally, we convert moles of carbon dioxide to grams using the molar mass of carbon dioxide, which is 44.01 g/mol.
Mass of carbon dioxide (CO2) = Moles of carbon dioxide × Molar mass
Mass of carbon dioxide = 0.828 moles × 44.01 g/mol ≈ 36.39 g
Therefore, when 11.9g of liquid hexane (C6H14) is combusted, approximately 36.39 grams of carbon dioxide gas (CO2) are formed.