a simple hwk question.. i don't understand what i need to do..

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
(Hint: The density of 1-butanol is 0.810 g/mL)

You only have to solve for the mass; everything else is irrelevant to the answer. I hate it when teachers give you a bunch of extra information that you do not need to solve a straight forward problem.

Density=mass/volume

So, solve for mass

density *volume=mass=(0.810g/mL)*(40.88mL)=33.1g of 1-butanol

notice that the mL's cancel out and you are only left with grams (g).

wait okay I figured it out till there... but then later I got this question and got stuck

How many moles of 1-butanol does this number of grams represent?

mols = grams/molar mass

To solve this problem, we need to use the given information and the concept of density to determine the mass of 1-butanol that has burned.

Let's break down the problem step by step:

Step 1: Identify the known values:
- Volume of 1-butanol burned: 40.88 mL
- Density of 1-butanol: 0.810 g/mL

Step 2: Determine the mass of 1-butanol burned:
We can use the formula: Mass = Volume x Density

Mass = 40.88 mL x 0.810 g/mL

Step 3: Calculate the mass of 1-butanol burned:
Multiply the volume (40.88 mL) by the density (0.810 g/mL) to get the mass:
Mass = 33.16 grams

Therefore, 33.16 grams of 1-butanol have burned.