How many atoms of nitrogen are present in 2.00 g of each of the following? (a) glycine, C2H5O2N?
Answer:
First we have to get the moles of glycine.
Its molecular weight is 75 g/mol
2.00 g / 75 = 0.0267 moles
There is 1 mole of N for each mole of glycine so we have 0.0267 moles of N
1 mole corresponds to 6.02 x 10^23 atoms
0.267 x 6.02 x 10^23 = 1.60 x 10^22 atoms of nitrogen
2.00 g/75 g/mole = 0.0267 mole
0.0267 mole x 6.02 x 10 e23 atom/mole = 1.61 x 10e22 atoms
i think you use the molar mass and avagadro's number.
so it would be 2.00g*(1 mol/75g)*(1 mol N/1 mol glycine)*(6.022x10^23atoms/1 mol N)=1.61x10^22atoms N
i hope thats right
take 2.00g and divided by the Molecular Weight of Glycine (or whatever compound you are finding) and then take the moles of Glycine that you found multiply it by the number of N in the compound and then multiply that to the Avogadro Number (6.022 * 10^ 23 )
2.00g/MW of Glycine * mole of N * Avogadro Number
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