how many grams of oxygen are required to burn 5.9g of C2H5OH?
Molar masses: C2H5OH= 45.06 g/mole
O2= 32.0 g/mole
Well, it appears that you're looking for the amount of oxygen needed to burn some C2H5OH. Let's see if we can calculate that, shall we?
First, we need to determine the molar ratio between C2H5OH and O2. From the balanced equation of the combustion reaction, we can see that for every C2H5OH molecule, we need 3 oxygen molecules.
Since we know the molar mass of C2H5OH is 45.06 g/mol, we can calculate the number of moles present in 5.9 grams. It will be 5.9 g / 45.06 g/mol = approximately 0.131 moles.
Since the molar ratio is 1:3, we can conclude that we would need 3 times the amount of moles of oxygen. Therefore, we need 0.131 moles x 3 = approximately 0.393 moles of O2.
Finally, to determine the mass of oxygen needed, we can multiply the number of moles by the molar mass of oxygen, which is 32.0 g/mol. So, 0.393 moles x 32.0 g/mol = approximately 12.6 grams of oxygen.
So there you have it! Around 12.6 grams of oxygen are required to burn 5.9 grams of C2H5OH. Just be careful not to let it get too heated, or you might end up with a fiery situation!
To calculate the number of grams of oxygen required to burn 5.9g of C2H5OH, we need to first determine the chemical equation for the combustion of C2H5OH. The balanced chemical equation for the combustion of C2H5OH is as follows:
C2H5OH + O2 → CO2 + H2O
From the equation, we can see that 1 mole of C2H5OH reacts with x moles of O2 to produce CO2 and H2O. Now, we can set up a proportion using the molar masses of C2H5OH and O2 to calculate the amount of O2 needed.
1 mole C2H5OH is equal to 45.06 g of C2H5OH.
1 mole O2 is equal to 32.0 g of O2.
Using the proportion:
(1 mole C2H5OH) / (45.06 g C2H5OH) = (x moles O2) / (32.0 g O2)
Now, we can solve for x, moles of O2, using cross-multiplication:
(1 mole C2H5OH) * (32.0 g O2) = (45.06 g C2H5OH) * (x moles O2)
32.0 g O2 = (45.06 g C2H5OH) * (x moles O2)
Dividing both sides by (45.06 g C2H5OH):
32.0 g O2 / 45.06 g C2H5OH = x moles O2
x = (32.0 g O2) / (45.06 g C2H5OH)
x ≈ 0.71 moles O2
Now, we can convert moles of O2 to grams of O2 by multiplying the moles by the molar mass:
Grams of O2 = (0.71 moles O2) * (32.0 g O2/mole)
Grams of O2 ≈ 22.7 g O2
Therefore, approximately 22.7 grams of oxygen are required to burn 5.9g of C2H5OH.