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Why is Knowledge of Composition Important?
Because everything in nature is either chemically or physically combined with other substances it is necessary to have knowledge of chemical composition. To know the amount of a material in a sample, you need to know what fraction of the sample it is.
• Examples that show the need to know about chemical composition:– the amount of sodium in sodium chloride for
dietary need– the amount of iron in iron ore for steel production– the amount of hydrogen in water for hydrogen
fuel– the amount of chlorine in Freon to estimate
ozone depletion
Counting Atoms by Moles• If we can find the mass of a particular number of atoms, we can use this
information to convert the mass of an element sample to the number of atoms in the sample.
• The number of atoms we will use is 6.022 x 1023 and we call this a mole– 1 mole = 6.022 x 1023 things, like 1 dozen = 12 things– The dozen and the mole make it easier to talk about large quantities– A mole can refer to anything, but we usually use it to talk about atoms,
molecules, and ions
• mole = number of particles equal to the number of atoms in 12 g of C-12
– 1 atom of C-12 weighs exactly 12 amu
– 1 mole of C-12 weighs exactly 12 g
• The number of particles in 1 mole is called Avogadro’s Number = 6.0221421 x 1023 (remember Avogadro’s # to 4 Sig. Figs.)
– 1 mole of C atoms weighs 12.01 g and has 6.022 x 1023 atoms
• the average mass of a C atom is 12.01 amu
Mass Number is Not the Same as Atomic Mass
• the atomic mass is an experimental number determined from all naturally occurring isotopes
• the mass number refers to the number of protons + neutrons in one isotope
– natural or man-made
Calculating Atomic Mass
Gallium has two naturally occurring isotopes: Ga-69 with mass 68.9256 amu and a natural abundance of 60.11% and Ga-71 with mass 70.9247 amu and a natural abundance of 39.89%. Calculate the atomic mass of gallium.
Solution: Convert the percent natural abundance into decimal form.
Ga-69 0.6011Ga-71 0.3989
Determine the Formula to Use Atomic Mass = (abundance1)∙(mass 1) + (abundance2)∙(mass 2) + ...Apply the Formula: Atomic Mass = 0.6011 (68.9256 amu) + 0.3989 (70.9247 amu) = 69.72
amu
Relationship Between Moles and Mass
• The mass of one mole of atoms is called the molar mass.
• The molar mass of an element, in grams, is numerically equal to the element’s atomic mass, in amu.
One mole
Converting Between Moles and Number of Atoms
A silver ring contains 1.1 x 1022 silver atoms. How many moles of silver are in the ring?
• Write down the given quantity and its units. Given: 1.1 x 1022 Ag atoms
• Write down the quantity to find and/or its units. Wanted: ? Moles
• Collect Needed Conversion Factors: 1 mole Ag atoms = 6.022 x 1023 Ag atoms
= 1.8266 x 10-2 moles Ag
= 1.8 x 10-2 moles Ag
moles atoms Ag 106.022
Ag mole 1atoms Ag 101.1
2322
Mole Relationships in Chemical Formulas
• since we count atoms and molecules in mole units, we can find the number of moles of a constituent element if we know the number of moles of the compound
Moles of Compound Moles of Constituents
1 mol NaCl 1 mole Na, 1 mole Cl
1 mol H2O 2 mol H, 1 mole O
1 mol CaCO3 1 mol Ca, 1 mol C, 3 mol O
1 mol C6H12O6 6 mol C, 12 mol H, 6 mol O
Masses of different substances that equal to one mole
Converting from Grams to Moles and Moles to Grams
How do you calculate the number of moles of sulfur in 57.8 g of sulfur?
S moles S g 2.063
S mole 1S g 57.8
= 1.80287 moles S = 1.80 moles S
Converting Between Grams and Number of Atoms
How many aluminum atoms are in an aluminum can with a mass of 16.2 g?
= 3.6159 x 1023 atoms Al
Sig. Figs. & Round: = 3.62 x 1023 atoms Al
Al mole 1
Al atoms 10022.6
Al g 26.98
Al mole 1Al g 6.21
23
Converting Between Grams and Moles of Compound
Calculate the mass (in grams) of 1.75 mol of water
OH g OH mol 1
OH g 18.02OH mol 1.75 2
2
22
= 31.535 g H2O
Sig. Figs. & Round: = 31.5 g H2O
Converting Between Grams and Number of Molecules
Find the mass of 4.78 x 1024 NO2 molecules?
= 365.21 g NO2
Sig. Figs. & Round: = 365 g NO2
2
2
223
22
24
NO mole 1
NO g 6.014
NO molec 10022.6
NO mole 1NO molec 1078.4
Converting Between Grams of a Compound and Grams of a Constituent ElementL-Carvone, (C10H14O), is found in spearmint oil. It has a pleasant odor and mint flavor. It is often added to chewing gum, liquors, soaps and perfumes. Find the mass of carbon in 55.4 g of carvone.
Molar Mass C10H14O = 10(atomic mass C) + 14(atomic mass H) + 1(atomic mass O)
= 10(12.01) + 14(1.01) + (16.00) = 150.2 g/mo
1 mole C10H14O = 150.2 g C10H14O
1 mole C10H14O 10 mol C
1 mole C = 12.01 g C
Solution Strategy “converting units” :
gC10H14O
C mol 1
C g 0112.OHC g 50.21
OHC mol 1
1410
1410
molC10H14O
molC
gC
OHC mol 1
C mol 10
1410
C mole 1
C g 2.011
OHC mol 1
C mol 10
OHC g 50.21
OHC mole 1OHC g 5.45
14101410
14101410
= 44.2979 g C
= 44.3 g C
Percent Composition• Percentage of each element in a compound by mass can be determined
from:1. the formula of the compound2. the experimental mass analysis of the compound
• The percentages may not always total to 100% due to rounding
100%wholepart
Percentage The mass percent tells you the mass of a constituent element in 100 g of the compound.The fact that NaCl is 39% Na by mass means that 100 g of NaCl contains 39 g Na.This can be used as a conversion factor:
100 g NaCl 39 g Na
Na g NaCl g 100
Na g 39 NaCl g NaCl g
Na g 39
NaCl g 100 Na g or
Example - Percent Composition from the Formula C2H5OH
1. Determine the mass of each element in 1 mole of the compound:Mass of Carbon = 2 moles C x (12.01 g) = 24.02 g
Mass of Hydrogen = 6 moles H x (1.008 g) = 6.048 g Mass of Oxygen = 1 mol O x (16.00 g) = 16.00 g
2. Determine the molar mass of the compound by adding the masses of the elements:
1 mole C2H5OH = 46.07 g
3. Divide the mass of each element by the molar mass of the compound and multiply by 100%:
52.14%C100%46.07g
24.02g 13.13%H100%
46.07g
6.048g
34.73%O100%46.07g
16.00g
Example – Percent Composition of Carvone if a 30.0 g sample contains 24.0 g of C, 3.2 g O and the rest H?
1. Determine the masses of all the elements in the sample
C = 24.0 g, O = 3.2 g
H = 30.0 g – (24.0 g + 3.2 g) = 2.8 g
2. Divide the mass of each element by the total mass of the sample then multiply by 100% to give its percentage
80.0%C100%30.0g
24.0g 11%O100%
30.0g
3.2g
9.3%H100%30.0g
2.8g
Hydrates
Hydrates are compounds that include water molecules as part of their structure
Examples include:
Na2CO3 • 10 H2O
NiCl2 • 6 H2O
What does this have to do with percent composition?
Percent Composition of Water
Let’s say we take 1.20 g of NiCl2 • x H2O (a hydrate)
With lots of heat from a Bunsen burner, we remove all the water and are left with 0.65 g of NiCl2. What is the percent composition of water in the hydrate?
(1.20 g of NiCl2 • 6 H2O) - (0.65 g of NiCl2) =
= 0.55 g H2O
% Comp. H2O = 0.55 g H2O (part) x 100% = 45% 1.20 g NiCl2 • x H2O (whole)
*We didn’t need to know the exact composition of the NiCl2 hydrate
% Composition and Formula
We find a compound and determine that it is composed of 31.2% nitrogen and 68.8% oxygen. What is the chemical formula of the compound?
For every 100. grams of material, there is 30.9 g N and 69.1 g O. We first convert to moles.
30.9 g N 1 mole N = 2.21 mole N 14.01 g
69.1 g O 1 mole O = 4.32 mole O 16.0 g
Examples: Empirical Formulas
Hydrogen PeroxideMolecular Formula = H2O2
Empirical Formula = HO
BenzeneMolecular Formula = C6H6
Empirical Formula = CH
GlucoseMolecular Formula = C6H12O6
Empirical Formula = CH2O
Finding an Empirical Formulafrom Experimental Data
A laboratory analysis of aspirin determined the following mass percent composition. Find the empirical formula.
C = 60.00%H = 4.48%
O = 35.53%
• Collect Needed Conversion Factors:
1 mole C = 12.01 g C
1 mole H = 1.01 g H
1 mole O = 16.00 g O
– calculate the moles of each element
Information
Given: 60.00 g C, 4.48 g H, 35.53 g O
Find: empirical formula, CxHyOz
Example:Find the empirical formula of aspirin with the given mass
percent composition.
C mol 996.4C g 12.01
C mol 1C g 00.60
H mol 44.4H g 1.01
H mol 1H g .484
O mol 220.2O g 16.00
O mol 1O g 5.523
This gives the formula ofC4.996H4.44O2.220. But, the formulamust have the atoms in whole number ratios!
Find the mole ratio by dividing by the smallest number of moles!
122.25
2.220
2.220
2.220
4.44
2.220
4.996
OHC
OHC
Multiplying the subscripts by 4 gives the final ratio!
C9H8O4
All these molecules have the same Empirical Formula. How are the molecules different?
Name Molecular
Formula
Empirical
Formula
glyceraldehyde C3H6O3 CH2O
erythrose C4H8O4 CH2O
arabinose C5H10O5 CH2O
glucose C6H12O6 CH2O
Molecular Formulas• The molecular formula is a multiple of the empirical formula
• To determine the molecular formula you need to know the empirical formula and the molar mass of the compound
Molar Massreal formula
Molar Massempirical formula
= factor used to multiply subscripts
Determine the Molecular Formula of Cadinene if it has a molar mass of 204 g/mol and an empirical formula of C5H8
Determine the empirical formula.Determine the molar mass of the empirical formula:
5 C = 60.05 g, 8 H = 8.064 g
C5H8 = 68.11 g
Divide the given molar mass of the compound by the molar mass of the empirical formula and round to the nearest whole number:
3g 11.68
g 204
Multiply the empirical formula by the factor above (3) to give the molecular formula:
(C5H8)3 = C15H24
Cadinenes: Sesquiterpenes found in junipers and cedars (oil of cade)