unit: chemical quantities determining the empirical formula from percent composition day 6 - notes
TRANSCRIPT
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Unit: Chemical QuantitiesDetermining the Empirical
Formula from Percent Composition
Day 6 - Notes
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After today, you will be able to…
•Calculate the empirical formulas for various compounds given their percent makeup
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Empirical Formula Determination from %
CompositionTo determine empirical formulas from % composition follow these steps:1.Assume 100.0g of the compound (change % into grams)2.Convert g moles for each element using molar mass3.Divide each mole answer by the smallest mole answer4.If you do not have a whole number, multiply by the smallest whole # to get a whole # ratio.5.Skip to this step if you already have a whole number ratio from #3. These whole #s are the subscripts for each element.
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To sum up these steps here is a poem for my favorite little
chemists:
“Percent to massMass to MolesDivide by small
Multiply by whole!”
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Example: What is the empirical formula for a compound that is 21.2% N, 6.10% H, 24.3% S, and 48.4%O?
21.2gN
6.10gH
24.3gS
48.4gO
1 mol N 14.01gN=
N2H8SO4
x 1.51
1 mol H 1.01gHx 6.04=
1 mol S 32.07gS
0.758
=x
x 1 mol O 16.00gO
3.03=
0.7580.7580.7580.758
=
=
=
=
2
7.97~
8
1
4
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Example: What is the empirical formula for a compound that is 69.8% Fe and 30.2% O?
69.8gFe
30.92gO
1 mol Fe
55.85gFe
=
Fe2O3
x 1.25
1 mol O 16.00gO
1.89=x
1.25
1.25
=
=
1
1.5
(2)
(2)
=
=
2
3
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Time to Practice!
Complete WS 6
HOMEWORK: