0
What is the total sample size (in grams) for a sample of ethanol (CH3CH2OH) which contains 3.36 g of oxygen?
Wiki User
∙ 7y ago
9.675 g
Since oxygen has an average atomic weight of 15.999 g/mol that would make it 0.21 moles of oxygen.
Ethanol has one atom of oxygen per molecule so that means 0.21 moles of ethanol.
Since ethanol has a molecular weight of 46.07 g/mole, 0.21 moles of ethanol would have a mass of 9.675 g.
Wiki User
∙ 7y ago
Wiki User
∙ 7y agoEthanol has the formula C2H6O and has a molar mass of 24+6+16 = 46 g/mol. If there are 3.36 g of O, then first convert that to moles: moles O = 3.36g x 1mol/16g = 0.21 moles O. Since each mole CH3CH2OH contains 1 mole O, there will be 0.21 moles CH3CH2OH. Mass of ethanol will thus be
0.21 moles ethanol x 46 g/mole ethanol = 9.66 grams
Wiki User
∙ 9y agoThe answer is 9,672 g ethanol.
Wiki User
∙ 7y ago6.09 grams, approx.
Add your answer:
Earn +20 pts
A Sample of a compound contains 64 g of copper and 16 g of oxygen what is the ratio of mass to copper of oxygen?
?
How many moles of sulfur are contained in a sample of CuSO4 that also contains 3.50 x 1023 oxygen atoms?
1
A 10g sample of the compound copper oxide contains 2.0 g of oxygenWhat mass of oxygen would a 30 g sample of the same compound contain?
it has 6 gram of copper
How many moles of ethanol C2H5OH are in a sample which weighs 39.2g?
Because the formula shows that each molecule of ethanol contains 2 atoms of carbon, 6* atoms of hydrogen, and 1 atom of oxygen, the gram molecular mass of one mole of ethanol is the sum of twice the gram atomic mass of carbon, 6 times the gram atomic mass of hydrogen, and the atomic mass of oxygen: 46.07. Therefore, 39.2 grams of ethanol constitutes 39.2/46.07 or 0.851 mole, to the justified number of significant digits. ________________ The subscript 5 immediately after the first appearance of the atomic symbol for hydrogen in the formula, plus the implied subscript 1 of the second appearance of the atomic symbol for hydrogen in the formula.
How many metric tons of oxygen are combined in a sample of pitchblende that contains 1.8 tons of uranium?
0.242 t of oxygen; but the value is only an approximate because the pitchblende is not only pure UO2.
A sample of ascorbic acid contains 1.50 of carbon and 2.00 of oxygen while another sample of ascorbic acid contains 6.35 of c. How many grams of oxygen does it contain?
23
If a 2.0mole sample of CH3CH2OH is completely burned how many moles of water will it produce?
2
A sample of nitric acid contains 50 HNO3 molecules How many oxygen atoms are in this sample?
150 (50 x 3)
A Sample of a compound contains 64 g of copper and 16 g of oxygen what is the ratio of mass to copper of oxygen?
?
Lipids test on brown paper?
If your asking whats the lipids test then it's: Heating a sample with ethanol, if it's cloudy then it contains high levels of lipids.
If a sample of air that has a total pressure of 150 ATM contains 69 oxygen what is the partial pressure of oxygen found within the air?
The pressure is 103,5 at.
How many moles of sulfur are contained in a sample of CuSO4 that also contains 3.50 x 1023 oxygen atoms?
1
What is the mass in grams of barium in a sample of barium phosphate that also contains 10.0g of oxygen?
This mass of barium is 32,33 g.
If a sample of ethanol has a volume of 60.0 ml what is the mass?
5
A 10g sample of the compound copper oxide contains 2.0 g of oxygenWhat mass of oxygen would a 30 g sample of the same compound contain?
it has 6 gram of copper
How is a sample oxygen different from a sample of a water?
Oxygen is just O and water is H2O
How many moles of ethanol C2H5OH are in a sample which weighs 39.2g?
Because the formula shows that each molecule of ethanol contains 2 atoms of carbon, 6* atoms of hydrogen, and 1 atom of oxygen, the gram molecular mass of one mole of ethanol is the sum of twice the gram atomic mass of carbon, 6 times the gram atomic mass of hydrogen, and the atomic mass of oxygen: 46.07. Therefore, 39.2 grams of ethanol constitutes 39.2/46.07 or 0.851 mole, to the justified number of significant digits. ________________ The subscript 5 immediately after the first appearance of the atomic symbol for hydrogen in the formula, plus the implied subscript 1 of the second appearance of the atomic symbol for hydrogen in the formula.
