The proportion by number of atoms in carbon dioxide is 1:2. The atomic weight of carbon is 12.011 and the atomic weight of oxygen is 15.9994. Therefore, the proportion by mass of carbon to oxygen in carbon dioxide is 12.011/(2 X 15.9994) = 0.37536 or 37.536 %, to the justified number of significant digits.
There are 2 moles of O per 1 mole of carbon dioxide (CO2). Use the molecular weight to find the mass of oxygen & mass of carbon dioxide.
2 moles of O * (16 g O / 1 mole O) = 32 g O
1 mole of CO2*(44 g CO2/1 mole CO2) = 44 g CO2
So the % oxygen in carbon dioxide by mass is:
32 g / 44 g * (100%) = 72.7%
By "Percentage by Msss" I assume you mean how much of the mass of Carbon Monoxide does Oxygen make up.
It's like this; one Carbon atom, one Oxygen atom. The atomic mass of carbon is about 12 AMUs (Atomic Mass Units) and Oxygen is about 16 AMUs. That gets up to 28 AMUs. 28 is close to a fourth of 100, so multiply 16 by four to get the approximate percentage: Oxygen makes up about 64% of Carbon Monoxide's mass.
atomic mass of Oxygen / molecule mass of carbon dioxide x 100 O / (Co2) x 100
33%
66%
Molecular weight of CO2 is about 44g (12g Carbon + 32g Oxygen *2 atoms Oxygen). So that means if you are presented with 44g CO2, that means there's 12g Carbon.
The molecular mass of CO is 28. The carbon percentage by mass is ~43%. Hence the oxygen percentage by mass is ~57%.
The gram molecular mass of hexane is 86.18. Therefore, 25.0 g of hexane constitute 25.0/86.18 or 0.290 moles. Each mole of hexane contains six carbon atoms and therefore will produce six molecules of carbon dioxide by burning in an excess of oxygen. 6 X 0.290 = 1.74 moles of carbon dioxide. The gram molecular mass of carbon dioxide is 44.00. Therefore, the mass of carbon dioxide produced will be 1.74 X 44.00 or 76.6 grams of carbon dioxide, to the justified number of significant digits.
If all of the quantities stated actually reacted, the law of the conservation of mass shows that the mass of carbon dioxide produced would be 40 - 18 or 22 grams.
1. Nitrogen. (It makes up 78% of the atmosphere) 2. Oxygen (21%) 3. Argon (1%) The local atmosphere may contain various amounts of water vapor by mass.
When methane burns, the carbon dioxide and water formed, equal the mass of the methane plus the mass of the oxygen.
law of multiple proportion
Molecular weight of CO2 is about 44g (12g Carbon + 32g Oxygen *2 atoms Oxygen). So that means if you are presented with 44g CO2, that means there's 12g Carbon.
11.0g
27.2 g
37.8
0.44g CO
This is the law om mass conservation.
This is the law om mass conservation.
44.010 g/mol You can sum up atomic weight of 1 carbon and 2 oxygen to this figure.
The molecular mass of CO is 28. The carbon percentage by mass is ~43%. Hence the oxygen percentage by mass is ~57%.
The gram molecular mass of hexane is 86.18. Therefore, 25.0 g of hexane constitute 25.0/86.18 or 0.290 moles. Each mole of hexane contains six carbon atoms and therefore will produce six molecules of carbon dioxide by burning in an excess of oxygen. 6 X 0.290 = 1.74 moles of carbon dioxide. The gram molecular mass of carbon dioxide is 44.00. Therefore, the mass of carbon dioxide produced will be 1.74 X 44.00 or 76.6 grams of carbon dioxide, to the justified number of significant digits.