I am assuming that the question is: what is the mass, in grams, of 9.93x1024 molecules of methanol (CH3OH).
For any question concerning mass and a chemical, we must find the molecular mass by adding the atomic masses from the periodic table:
C=12.0g
4H= 4 x 1.01 = 4.04g
O=16.0g
Total: 32.0g/mole
Now, how many moles is 9.93x1024 molecules, if one mole is 6.02x1023? (9.93x1024 ) / (6.02x1023) = 15.5 moles.
So, 15.5 moles x 32.0g/mole = 496g.
9,85x10 to the 24 of methanol (CH3OH) molecules have a mass of 52,405 g.
9.32*1024 (molec's CH3OH) / 6.022*1023 (molec's.mol−1 CH3OH) * 32.04 (g mol−1 CH3OH) = 495.8 g = 496 g CH3OH
9.32*1024 (molec's CH3OH) / 6.022*1023 (molec's.mol−1 CH3OH) * 32.04 (g mol−1 CH3OH) = 495.8 g = 496 g CH3OH
192.678 grams CH3OH
7,207 g methanol are needed.
9,85x10 to the 24 of methanol (CH3OH) molecules have a mass of 52,405 g.
9.32*1024 (molec's CH3OH) / 6.022*1023 (molec's.mol−1 CH3OH) * 32.04 (g mol−1 CH3OH) = 495.8 g = 496 g CH3OH
9.32*1024 (molec's CH3OH) / 6.022*1023 (molec's.mol−1 CH3OH) * 32.04 (g mol−1 CH3OH) = 495.8 g = 496 g CH3OH
9.18x10^24 molecules CH3OH x 1 mole/6.02x10^23 molecules x 32 g/mole = 488 g (to 3 sig figs)
192.678 grams CH3OH
The mass is 483,62 g.
CH3OH + NH3 → CH3NH2 + H2O 32 g of methanol reacts with 17.0 g ammonia 21 g of CH3OH react with 11.0 g NH3
8.20g of carbon monoxide, how many grams of methanol will be produced?
7,207 g methanol are needed.
The answer is 50,196 g.
The answer is 9.6 grams.
The simplest form of the molecular formula for methanol {note corrected spelling} is CH4O, and its gram molecular mass is 32.04. By definition therefore, a mass of Avogadro's Number of molecules contains 32.04 grams. Avogadro's Number is about 6.022 X 1023. Therefore, 9.47 X 1024 molecules of methanol contains [(9.47 X 1024)/(6.022 X 1023)]32.04 or 504 grams, to the justified number of significant digits.