how many grams of product can be made from 1 mol of ethanol
To determine how many grams of product can be made from 1 mole of ethanol, we need to know the molecular mass of the product we are interested in.
Let's assume we are interested in the product formed by complete combustion of ethanol, which is carbon dioxide (CO2) and water (H2O). The balanced chemical equation for the complete combustion of ethanol is:
C2H5OH + 3O2 -> 2CO2 + 3H2O
From the balanced equation, we can see that for every 1 mole of ethanol (C2H5OH), we get 2 moles of carbon dioxide (CO2) and 3 moles of water (H2O).
Next, let's calculate the molecular mass of ethanol, carbon dioxide, and water.
The molecular mass of ethanol (C2H5OH) is:
C = 12.01 g/mol
H = 1.01 g/mol (5 hydrogens)
O = 16.00 g/mol (1 oxygen)
So the molecular mass of ethanol is:
(2 * 12.01) + (6 * 1.01) + 16.00 = 46.07 g/mol
The molecular mass of carbon dioxide (CO2) is:
C = 12.01 g/mol (1 carbon)
O = 16.00 g/mol (2 oxygens)
So the molecular mass of carbon dioxide is:
12.01 + (2 * 16.00) = 44.01 g/mol
The molecular mass of water (H2O) is:
H = 1.01 g/mol (2 hydrogens)
O = 16.00 g/mol (1 oxygen)
So the molecular mass of water is:
(2 * 1.01) + 16.00 = 18.02 g/mol
Now, using the molar ratios from the balanced equation, we can calculate how many grams of carbon dioxide and water are produced from 1 mole of ethanol.
For carbon dioxide (CO2):
1 mole of ethanol produces 2 moles of CO2
So, the mass of CO2 produced from 1 mole of ethanol is:
(2 * 44.01) = 88.02 g
For water (H2O):
1 mole of ethanol produces 3 moles of H2O
So, the mass of H2O produced from 1 mole of ethanol is:
(3 * 18.02) = 54.06 g
Therefore, when 1 mole of ethanol undergoes complete combustion, it will produce 88.02 grams of carbon dioxide and 54.06 grams of water.