Download - Percent composition and empirical formulas
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Percent composition and empirical formulas
No matter how great and destructive your problems may seem now, remember, you've
probably only seen the tip of them
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An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
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An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
• Chlorine atoms are heavier than sodium atoms.
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An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
• Chlorine atoms are heavier than sodium atoms. By mass:
• Na=22.99g/mol
• Cl=35.45g/mol
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An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
• Chlorine atoms are heavier than sodium atoms. By mass:
• %Na=22.99g/58.44 g x 100%
• %Cl=35.45g/58.44 g x 100%
![Page 6: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/6.jpg)
An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
• Chlorine atoms are heavier than sodium atoms. By mass:
• %Na=22.99g/58.44 g x 100%
• %Cl=35.45g/58.44 g x 100%FM of NaCl !
![Page 7: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/7.jpg)
An example.
• You could claim that NaCl is half sodium and half chlorine—one of each.
• Chlorine atoms are heavier than sodium atoms. By mass:
• %Na=22.99g/58.44 g x 100%=39.34% and
• %Cl=35.45g/58.44 g x 100%=60.66%
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Definition
• % composition of a compound:
• % A= mass A in the compound x 100%
mass of the compound
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PS
• All of the %’s add up to 100%
• The %’s are constant, no matter how much of the substance!
• (AKA: the law of definite proportions)
![Page 10: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/10.jpg)
Try it.
• What is the percent composition of CaBr2?
![Page 11: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/11.jpg)
Try it.
• What is the percent composition of CaBr2?
(FM=199.88g/mol)
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Try it.
• What is the percent composition of CaBr2?
(FM=199.88g/mol)
• %Ca=40.08g/199.88 g x 100% and
• %Br=2 x 79.90g/199.88 g x 100%
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Try it.
• What is the percent composition of CaBr2?
(FM=199.88g/mol)
• %Ca=40.08g/199.88 g x 100%=20.05% and
• %Br=2 x 79.90g/199.88 g x 100%=79.95%
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Practice
• ? %comp of:
1) CaO
2) Na3N
3) Al2(SO4)3
4) NaNO3
5) NaNO2
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Practice
• ? %comp of:
1) CaO 71.47%Ca 28.53%O
2) Na3N 83.12%Na 16.88%N
3) Al2(SO4)3 15.77%Al 28.11%S 56.12%O
4) NaNO3 27.05%Na 16.48%N56.47%O
5) NaNO2 33.32%Na 20.30%N46.38%O
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So what?
• Iron (II) oxide is 77.73% iron.
• Iron (III) oxide is 69.94% iron.
• An iron oxide that contains 16.09 g of iron and 6.91 g of oxygen has to be…
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So what?
• Iron (II) oxide is 77.73% iron.
• Iron (III) oxide is 69.94% iron.
• An iron oxide that contains 16.09 g of iron and 6.91 g of oxygen has to be…
Uhh… 16.09/(16.09 +6.91) x 100%=…
![Page 18: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/18.jpg)
So what?
• Iron (II) oxide is 77.73% iron.
• Iron (III) oxide is 69.94% iron.
• An iron oxide that contains 16.09 g of iron and 6.91 g of oxygen has to be…
Iron (III) oxide
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On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
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On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
• 8.39 g Ti
• 5.61 g O
![Page 21: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/21.jpg)
On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
• 8.39 g Ti x 1mol Ti/47.90 g
• 5.61 g O x 1mol O/16.00 g
![Page 22: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/22.jpg)
On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
• 8.39 g Ti x 1mol Ti/47.90 g=.175 mol Ti
• 5.61 g O x 1mol O/16.00 g=.350 mol O
• Ti.175O.350
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On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
• 8.39 g Ti x 1mol Ti/47.90 g=.175 mol Ti
• 5.61 g O x 1mol O/16.00 g=.350 mol O
• Ti.175O.350 Ti.175/.175O.350/.175
![Page 24: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/24.jpg)
On the other hand…
• A sample contains 8.39 g Ti and 5.61 g O. What is the formula of this compound?
• 8.39 g Ti x 1mol Ti/47.90 g=.175 mol Ti
• 5.61 g O x 1mol O/16.00 g=.350 mol O
• Ti.175O.350 Ti.175/.175O.350/.175 TiO2
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Try it.
• A sample contains 2.6366 g C, 0.4425 g H, and 3.5122 g O. What is the empirical formula of this compound?
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Try it.
• A sample contains 2.6366 g C, 0.4425 g H, and 3.5122 g O. What is the empirical formula of this compound?
CH2O
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Try it.
• A sample contains 35.378g C, 5.938 g H, and 31.418 g O. What is the formula of this compound?
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There are two things to watch out for:
1) What if the smallest number is not 1?
2) What if the simplest whole number ratio is smaller than the molecule?
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol
• 1.60 g S /32.06 g/mol
• 1.20 g O/16 g/mol
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol=.0500 mol Na
• 1.60 g S /32.06 g/mol=.0500 mol S
• 1.20 g O/16 g/mol= .0750 mol O
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol=.0500 mol Na• 1.60 g S /32.06 g/mol=.0500 mol S• 1.20 g O/16 g/mol= .0750 mol O
Na.05S.05O.075
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol=.0500 mol Na• 1.60 g S /32.06 g/mol=.0500 mol S• 1.20 g O/16 g/mol= .0750 mol O
Na.05S.05O.075 NaSO1.5
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol=.0500 mol Na• 1.60 g S /32.06 g/mol=.0500 mol S• 1.20 g O/16 g/mol= .0750 mol O
Na.05S.05O.075 NaSO1.5
Don’t try to round the decimal away!
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1) What if the smallest number is not 1?
• A sample contains 1.15 g Na, 1.60 g S, and 1.20 g O.
• 1.15 g Na/22.99g/mol=.0500 mol Na• 1.60 g S /32.06 g/mol=.0500 mol S• 1.20 g O/16 g/mol= .0750 mol O
Na.05S.05O.075 NaSO1.5 Na2S2O3
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• Al.17O.255
• C.89H1.18
• C1.58H 4.22 O1.58
• C1.90H2.38Cl2.38
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• Al.17O.255AlO1.5
• C.89H1.18 CH1.33
• C1.58H 4.22 O1.58 CH2.67O
• C.190H2.38Cl2.38 CH1.25Cl1.25
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• Al.17O.255AlO1.5 Al2O3
• C.89H1.18 CH1.33 C3H4
• C1.58H 4.22 O1.58 CH2.67O C3H 8 O3
• C.190H2.38Cl2.38 CH1.25Cl1.25 C4H5Cl5
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Try it.
• A sample contains 2.6366 g C, 0.4425 g H, and 3.5122 g O. What is the empirical formula of this compound?
CH2O• If we know that the FM of the compound is about
60g/mol, what is the molecular formula?
• FM(CH2O)=30g/mol
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Try it.
• A sample contains 2.6366 g C, 0.4425 g H, and 3.5122 g O. What is the empirical formula of this compound?
CH2O• If we know that the FM of the compound is about
60g/mol, what is the molecular formula?
• FM(CH2O)=30g/mol x 2=60 g/mol
• CH2O x 2= C2H4O2
![Page 41: Percent composition and empirical formulas](https://reader035.vdocument.in/reader035/viewer/2022062309/56814957550346895db6aa7d/html5/thumbnails/41.jpg)
Try it.
• A sample contains 2.6366 g C, 0.4425 g H, and 3.5122 g O. What is the empirical formula of this compound?
CH2O• If we know that the FM of the compound is about
60g/mol, what is the molecular formula?
C2H4O2