1-butanol (shown below) burns in the presence of oxygen to give off carbon dioxide and water by the following reaction:

C4H9OH + 6 O2 ==> 4 CO2 + 5 H2O
If 40.88 mL of 1-butanol burns completely, how many grams of 1-butanol have burned? grams

=33.1

bu then
Now, How many moles of 1-butanol does this number of grams represent?

molar mass/grams? my answer says it's wrong though... which is 8.03

mols = grams/molar mass

To determine the number of grams of 1-butanol that have burned, you need to use the given volume and the density of 1-butanol.

1. First, you need to find the density of 1-butanol. The density of 1-butanol is approximately 0.810 g/mL.

2. Next, you can calculate the mass of 1-butanol using the formula: mass = volume * density. Plug in the values: mass = 40.88 mL * 0.810 g/mL = 33.10 grams. Therefore, 33.10 grams of 1-butanol have burned.

Now, to find the number of moles of 1-butanol, you can use the molar mass of 1-butanol. The molar mass of 1-butanol (C4H9OH) is given by:

(4 * atomic mass of Carbon) + (10 * atomic mass of Hydrogen) + (1 * atomic mass of Oxygen).

To find the atomic masses of carbon, hydrogen, and oxygen, you can refer to the periodic table. The atomic masses are approximately 12.01 g/mol, 1.01 g/mol, and 16.00 g/mol, respectively.

3. Calculate the molar mass: (4 * 12.01 g/mol) + (10 * 1.01 g/mol) + (1 * 16.00 g/mol) = 74.12 g/mol.

Now, to find the number of moles of 1-butanol, divide the mass by the molar mass:

moles = mass / molar mass = 33.10 g / 74.12 g/mol ≈ 0.446 mol

Therefore, the number of moles of 1-butanol represented by 33.10 grams is approximately 0.446 moles.