CO2 has a molecular weight of 44.01 g/mol, so 924 grams is equivalent to 20.99522835719155 moles.
Avogadro's number gives the number of units in one mole of any substance (defined as its molecular weight in grams), equal to 6.022140857 × 10 to the 23 (Note the units may be electrons, atoms, ions, or molecules, depending on the nature of the substance).
Thus the number of molecules in 924 grams of Carbon Dioxide is = 20.99522835719155 times 6.022140857 × 10 to the 23. = 126.4362224918882 × 10 to the 23
One mole of 12C has a mass of 12.00000 grams (exactly, by definition).One mole of 13C has a mass of 13.00335 grams.One mole of 14C has a mass of 14.00324 grams.One mole of natural carbon - i.e. a sample with the ration of isotopes equal to that in nature - has a mass of 12.0107 grams.
The density of O2 is 31.9988 grams per mole, meaning there are 0.143 grams and 4.47 mmols present. The density of NH3 is 17.0305 grams per mole, giving 4.09 mmols of ammonia. This means that they have approximately the same number of mmoles, thus the same number of molecules.
One mole is what 6.022x1023 molecules of an element masses. Example: One mole of Carbon equals 12.01 grams.
550 g of nitrogen dioxide is equal to 11,94 moles.
Each glucose molecule contains 6 carbon atoms. Thus we need 18 molecules of CO2 to make 3 molecules of glucose.
By experiment, a gram mole of any substance contains about 6.022 X 1023 molecules of the substance. The gram molecular mass of carbon dioxide, with the formula CO2, is about 44.01. Therefore 485 grams of carbon dioxide contains 485/44.01 or about 11.02 gram molecular masses. The formula for carbon dioxide shows that each molecule contains one carbon atom. Therefore, 11.02 moles of carbon dioxide contains 11.02 X 6.022 X 1023, or about 4.00 X 1024 atoms of carbon, to the justified number of significant digits.
The gram molecular mass of carbon dioxide is about 44.01 grams. By definition, this value is the number of grams of carbon dioxide that contains Avogadro's Number ("AN") of molecules. Avogadro's Number is about 6.022 X 10^23. Therefore the number of molecules in 1 gram is (1/44.01)(AN) or 2 X 10^21 molecules, to the justified number of significant digits.
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
72 grams SO2 (1 mole SO2/64.07 grams)(6.022 X 1023/1 mole SO2) = 6.8 X 1023 molecules of sulfur dioxide ============================
22 grams carbon dioxide (0.5 moles)
6 grams
The mass of carbon dioxide is 141,2 g.
It depends on the substance. If you have for example, 12 grams of Carbon-12. Then you have 1 mole of carbon 12 which is 6.02 * 1023 molecules of the element, which is equal to 12 grams. One mole of a compound or element is equal to that element's atomic mass in grams.
11 grams because all is reacted and there is no reactant left over, although if there were only 3 grams of carbon there would have to be 6 grams of oxygen for this to be viable as carbon dioxide is CO2 so the question asked was itself wrong.
Look up the molecular weight of carbon dioxide in the periodic table. The formula for carbon dioxide is CO2, which means one atom of carbon and two atoms or oxygen per molecule of carbon dioxide. Carbon has molecular weight of 12. Oxygen molecular weight is 16. Total 12+16+16= 44 11 grams/44 grams/mole=0.25 moles of carbon The grams of water and combustion of 7.5 grams are totally irrelevant. They are only given to possibly confuse you.
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One mole of 12C has a mass of 12.00000 grams (exactly, by definition).One mole of 13C has a mass of 13.00335 grams.One mole of 14C has a mass of 14.00324 grams.One mole of natural carbon - i.e. a sample with the ration of isotopes equal to that in nature - has a mass of 12.0107 grams.