MOLES Mole: A collection of objects A collection of Avogadro’s number of objects Avogadro’s...
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Transcript of MOLES Mole: A collection of objects A collection of Avogadro’s number of objects Avogadro’s...
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MOLES
Mole: A collection of objects
A collection of Avogadro’s number of objects
Avogadro’s number 6.022 * 1023 AtomsParticlesIonsCationsAnionsMoleculesFormula Units
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Mole Ratio
The coefficient in front of each component in a balanced equation
2 Al (s) + 6 HCl (aq) ----- 2 AlCl 3 (aq) + 3 H2 (g)
This states: 2 moles of Al reacts w/ 6 moles HCl to produce2 moles AlCl3 and 3 moles H2 gas
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MOLE CALCULATIONS
One mole of helium atoms …. ….. is a number
6.022 * 1023 Helium atoms
One mole of argon atoms …. ….. is a number
6.022 * 1023 Argon atoms
….. has a mass ….. has a mass
4.00 grams 39.9 grams
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RECAP: 1 mol of “anything” contains 6.022*1023 “parts” Elements on p.table = I mol
Molar mass (mass/1 mol)1. Elements - decimal # on p.table Ti 47.87 amu or g2. Molecules/Cmpd - sum of mass of all elements
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MOLES
MASS
Mul
tiply
by D
ivid
e
by
mass = 1 mole
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Given mass, find moles
How many moles are in 345.6 g NaNO3 ?
Step 1: find formula wt. of NaNO3
1 Na = 23.0 g1 N = 14.0 g3 O = 3 * 16.0 = 48.0 g
1 mole of NaNO3 = 85.0 g
Step 2 : Find # of moles Use factor-label method
Conversion * 1
Given g 85.0
mole 1 * 1
g 345.64.07 moles NaNO3
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Given moles, find mass
How many grams are in 0.6 moles N2O ?
Step 1: find molecular wt. of N2O
2 N = 2 * 14.0 = 28.0 g1 O = 16.0 g
1 mole of N2O = 44.0 g
Step 2 : Find mass Use factor-label method
mol 1
g 44.0 * 1moles 0.6 26.4 g N2O
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MOLES
NUMBER of PARTICLES
6.02*1023
Avogadro’s N
umber
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Given moles, find # molecules
How many molecules are in 1.6 moles oxygen?
Step 1: Recognize that mass does not apply here. But Avogadro’s # is used
Step 2 : Find # molecules Use factor-label method
mol 1
10 * 6.02 * 1
moles 1.6 molecules239.63 * 1023 molecules O2
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Given # atoms, find moles
How many moles are in 3.01 *1012 atoms of Chromium?
Step 1: Recognize that mass does not apply here. But Avogadro’s # is used
Step 2 : Find # moles Use factor-label method
10 * 6.02
mole 1 * 1
atoms 10 * 3.01atoms23
125.00 * 10-12 mols Cr
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MOLES
MASSNUMBER of PARTICLES
Mul
tiply
by D
ivid
e
by
mass = 1 mole
6.02*1023
There is not a direct relationshipbetween MASS and PARTICLES
Avogadro’s N
umber
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Given # formula units, find grams
2 Step Conversion ProblemWill need to use MASS at some point in the problem
How many grams are in 1.208 * 1024 formula units AgCl ?
Step 1: find formula wt. of AgCl
1 Ag = 107.9 g1 Cl = 35.5 g
1 mole of AgCl = 143.4 g
Step 2 : Find moles Use factor-label method
mol 1
g 143.4 * units 10 * 6.02
mol 1 * 1
units 10*1.20823
24288 g AgCl
Converts formula units to MOLES THEN
Converts moles to MASS
Step 3 : Find mass
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Given grams, find # atomsWill need to use MASS at some point in the problem
2 Step Conversion Problem
How many atoms are in 128.0 grams of Mercury ?
Step 1: find molar mass of Hg
1 mole of Hg = 200.6 g
Step 2 : Find moles Use factor-label method
mol 1
atoms 10 * 6.02 *
g 200.6mol 1
* 1
g 128.0 23
3.84*1023 atoms Hg
Converts mass to MOLES THEN
Converts moles to ATOMS
Step 3 : Find atoms
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PROBLEM What is the formula weight of sodium carbonate, Na2CO3. This is an industrial chemical used inmaking glass.
SOLUTION
2 Na
1 C
3 O
2 * 23.0 = 46.0
1 * 12.0 = 12.0
3 * 16.0 = 48.0
106.0 g
Also, equivalent to 1mole of a substance
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Sodium Phosphate (aq) + Barium Nitrate (aq) ------ Barium Phosphate (s) + Sodium Nitrate (aq)
Na3PO4 (aq) + Ba(NO3)2 (aq) ----- Ba3(PO4)2 (s) + NaNO3 (aq) 3 632
BALANCE EQUATIONS “STOICHIOMETRY”
Al + HCl ---- AlCl3 + H23 36 22
Aluminum (s) + Hydrochloric Acid (aq) ----------> Aluminum Chloride (aq) + Hydrogen (g)
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MASS - MASS CALCULATIONS & LIMITING REAGENT
Solid calcium metal burns in air (oxygen) to form a calcium oxide cmpd. Using 4.20 g Ca & 2.80 g O2 how much pdt is made? Find 1) grams of pdt made from g of Ca 2) grams of pdt made from g of O2
3) limiting reagent 4) how much pdt can be made 5) % yield if 3.85 g produced
PLAN: Need ------> balanced chem. rxn
g Ca -----> mols Ca -----> mols pdt ------> g pdtM g Ca coeff X pdt/Y react M g pdt
STEPS:
Ca(s) + O2(g) -------> CaO(s)2 2
M g Ca M g O2 coeff X pdt/Y react M g pdt40.1 g Ca:CaO 2:2 56.1 g 32.0 g O2:CaO 1:2
(same steps converting oxygen)
(amts of 2 reactants given: limiting reactants)
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2 Ca(s) + O2(g) -------> 2 CaO(s)
4.20 g 2.80 g X g
M g : 40.1g 56.1 gCoeff : 2 1 2mols :
CaO g 5.89 mol 1
g 56.1mol) 105.0(CaO mol 105.0
Ca mol 2
CaO mol 2
g 40.1
mol 1Ca g 20.4 )1
0.105 0.105
CaO g 82.9mol 1
g 1.56mol 175.0CaO mol 175.0
O mol 1
CaO mol 2
g 32.0
mol 1O g 80.2 )2
22
0.0875 0.175
5.89 g 9.82 g
3) limiting reagent: Which produced the least amt-- Ca or O2?Ca ---> CaO = 5.89 g O2 ---> CaO = 9.82 gCa, limiting reagent
4) how much pdt can be made: 5.89 g CaO
5) % yield= 100
amountltheoretica
amountactual % 65.4 100g 89.5
g 85.3
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RECAP: -- Balanced chem. equation -- then, GIVEN USE FIND grams Molar Mass mols mols coeff mols mols Molar Mass gramslimiting reagent: the reactant that produces the least amt of moles or mass of a specific pdt