OK.
You are correct that
moles = grams/molar mass
AND
atomic mass in grams/6.022 x 10^23 = mass of one atom.
# molecules in 0.334 g ethane.
Convert to moles.
moles = grams/molar mass.
0.334/30 = ?? I estimated the 30; you need to confirm it and change if appropriate.
We know 1 mole of anything contains 6.022 x 10^23 molecules; therefore,
# molecules = 6.022 x 10^23 molecules/mole x ??moles from above = # molecules.
By the way, I notice throughout the post that you are omitting an h in WHERE which made it a little difficult to understand when I first read it as WERE.
I have realized I don't understand Avagado's number at all
My book shows me this diagram instead of just providing a simple formulas that makes no sense at all
here is what I have made sense of so far
(6.022 x 10^23 atoms/mol)(mass of element) = molecular mass
were molecular mass is just the mass number off the periodic table with units g/mol
solving for mass of element will provide the units of g/atoms which makes perfect sense so I think I have this part down if you want to be gramtically correct g/atom
Here's a sample problem in which I would use this equation: Calculate the mass in grams of a single carbon-12 atom
(12.0 g/mol)/(6.022 x 10^23 atoms/mol) = 1.993 x 10^-23 g/atom
Also
(molecular mass)n = mass of element
were mass is the mass of the element given in g and molecular mass is the mass number from periodic table with units g/mol
n is the number of moles
solving for n provides moles for the final unit so I think I get this equation down
Example probelm: How many moles of He atoms are in 6.46 g?
(6.46 g)/(4.003 g/mol) = 1.61 mol
I'm trying to solv this problem
How mnay molecules of ethane C2H6 are present in .334 g of C2H6?
Now I don't now how to solve the problem I posted above were its asking me for molecules
Can someone just show me the apropriate formulas as I'm just reading this crazy diagram and trying to make sense of it and deriving the formulas from it myself... thanks
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