Ethanol is the active ingredient of alcoholic beverages. It is also s a possible replacement for gasoline. The complete combustion of ethanol forms carbon dioxide and water.
CH3CH2OH + O2 => CO2 + H2O
Balance the equation. What mass of carbon dioxide is formed by the complete combustion of 775 g of ethanol?
CH3CH2OH + 3O2 => 2CO2 + 3H2O
CH3CH2OH is
2*C = 24 +
6*H = 6 +
1*O = 16 = 46 grams/mol
so that is 775/46 = 16.85 mols of ethanol
so we would get 2*16.85 = 33.7 mols of CO2
CO2 = 12+32 = 44 grams/mol
33.7 *44 = 1483 grams of CO2
Oh my, greenhouse galore
To balance the equation, you need to make sure that there is an equal number of atoms on both sides. Here is how you balance the equation:
CH3CH2OH + 3O2 => 2CO2 + 3H2O
Now, you can see that there are two carbon dioxide molecules produced for every one ethanol molecule.
To find the mass of carbon dioxide formed by the complete combustion of 775 g of ethanol, you need to use stoichiometry. The molar mass of ethanol (C2H5OH) is approximately 46.07 g/mol, and the molar mass of carbon dioxide (CO2) is approximately 44.01 g/mol.
First, calculate the number of moles of ethanol:
Moles of ethanol = mass of ethanol / molar mass of ethanol
Moles of ethanol = 775 g / 46.07 g/mol
Next, use the balanced equation to determine the ratio of moles of carbon dioxide to moles of ethanol. From the balanced equation, you can see that 2 moles of CO2 are produced for every 1 mole of ethanol.
Now, multiply the moles of ethanol by the conversion factor:
Moles of CO2 = moles of ethanol * (2 moles of CO2 / 1 mole of ethanol)
Finally, calculate the mass of carbon dioxide:
Mass of CO2 = moles of CO2 * molar mass of CO2
Inserting the values into the equations:
Moles of ethanol = 775 g / 46.07 g/mol = 16.81 mol
Moles of CO2 = 16.81 mol * (2 mol CO2 / 1 mol ethanol) = 33.62 mol
Mass of CO2 = 33.62 mol * 44.01 g/mol = 1,480.62 g
Therefore, the mass of carbon dioxide formed by the complete combustion of 775 g of ethanol is approximately 1,481 g.
To balance the equation for the combustion of ethanol, we need to ensure that the number of atoms of each element is the same on both sides of the equation.
The balanced equation is:
C2H6O + 3O2 => 2CO2 + 3H2O
From the balanced equation, we can see that 1 mole of ethanol reacts with 2 moles of carbon dioxide.
To find the number of moles of ethanol, we can use its molar mass:
Molar mass of ethanol (C2H6O) = 2(12.01 g/mol) + 6(1.01 g/mol) + 16.00 g/mol
= 46.07 g/mol
Number of moles of ethanol = Mass of ethanol / Molar mass of ethanol
= 775 g / 46.07 g/mol
≈ 16.82 mol
Since 1 mole of ethanol produces 2 moles of carbon dioxide, the number of moles of carbon dioxide formed will be:
Number of moles of carbon dioxide = 2 moles of carbon dioxide/mol of ethanol × 16.82 mol
≈ 33.64 mol
Finally, to find the mass of carbon dioxide, we can use its molar mass:
Molar mass of carbon dioxide (CO2) = 12.01 g/mol + 2(16.00 g/mol)
= 44.01 g/mol
Mass of carbon dioxide = Number of moles of carbon dioxide × Molar mass of carbon dioxide
= 33.64 mol × 44.01 g/mol
≈ 1480.56 g
Therefore, approximately 1480.56 g of carbon dioxide is formed by the complete combustion of 775 g of ethanol.