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Molar Mass & Conversions
The Mole
mole (mol)- SI Unit for the amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12.
•A unit of counting, like the dozen.
Avogadro’s NumberAvogadro’s Number - the number of
particles in exactly one mole of a pure substance.
1 mole = 6.0221415 X 1023
1 mol = 6.022 x 1023
Amedeo Avogadro
Atomic Massatomic mass - the mass of one mole of an
atom•Atomic mass is expressed in atomic mass
units (amu) or (u) or g/mol.•Can be found on the periodic table.•All atomic masses are based on the
atomic mass of carbon-12 being 12 amu.
Molar Mass
molar mass - the mass of one mole of a pure substance.
•Molar mass is written in units of amu or g/mol.
Atomic mass vs. Molar mass
•atomic mass - the mass of one mole of an atom.
•molar mass - the mass of one mole of a pure substance.
Atomic Mass vs. Molar Mass
Example Atomic Mass Molar Mass
Na
Ag
C
O
22.99 g/mol 22.99 g/mol
107.87 g/mol
107.87 g/mol
12.01 g/mol 12.01 g/mol
16.00 g/mol 16.00 g/mol
Molar Mass of Compounds
Compound Molar Mass
H2O
C6H12O6
NaCl
Cl2
(NH4)3PO4
CuSO4·5H2O
18.02 g/mol
180.18 g/mol58.44 g/mol
70.90 g/mol
149.12 g/mol249.72 g/mol
Introduction to Molar Conversions
Amount Mass
1 mol O2
½ mol O2
2 mol O2
3 mol O2
32.00 g
16.00 g
64.00 g
96.00 g
Grams to MolesConverting grams to moles: divide by molar mass.
1. How many moles of Ca are in 5.00g of Ca?
2. How many moles of H2O are in 36.0g of H2O?
3. How many moles of AgNO3 are in 124.5g of AgNO3?
1 mol Ca5.00g Ca x =
40.08 g Ca0.125 mol Ca
22
2
1 mol H O36.0 g H O x =
18.02 g H O 22.00 mol H O
33
3
1 mol AgNO124.5 g AgNO x =
169.88 g AgNO0.7329
3mol AgNO
Moles to Grams
Converting from moles to grams: multiply by molar mass.
1. What is the mass in grams of 2.25 moles of Fe?
2. What is the mass in grams of 0.896 moles of BaCl2?
55.85 g Fe2.25 mol Fe x =
1 mole Fe 126 g Fe
2187 g BaCl
Types of Particles•Atoms – C, Cu, He
•Molecules – O2, C12H22O11, CO2 (all nonmetals in the formula)
•Formula units – NaCl, CaCl2, Mg(NO3)2 (includes a metal in the formula)
Particles to MolesConverting particles to moles: divide by Avogadro's Number.
1. How many moles of Pb are in 1.50 X 1025 atoms of Pb?
2. How many moles of CO2 are in 6.78 X 1021 molecules of CO2?
2.49 x 101 moles Pb
1.13 x 10-2 moles CO2
Moles to ParticlesConverting moles to atoms: multiply by Avogadro's Number.
1. How many molecules of NO are in 0.87 moles of NO?
2. How many formula units of NaI are in 2.50 moles of NaI?
5.2 x 1023 molecules NO
1.51 x 1024 formula units NaI
Grams to Moles to Particles
Example: How many molecules of N2 are in 57.1g of N2?
257.1 g N x 2
2
1 mol N
28.02 g N
232
2
6.02 x 10 molecules Nx
1 mol N
242= 1.23 x 10 molecules N
Particles to Moles to Grams
Example: How many grams of NaF are in 7.89 X 1024 formula units of NaF?
247.89 x 10 f.un. NaF x 23
1 mol NaF
6.02 x 10 f.un. NaF
41.99 g NaFx
1 mol NaF
= 550. g NaF
Atoms to Moles to Grams
Tough Example:
How many total atoms are in 235 g of CO2?
9.64 x 1024 total atoms
The Mole Bridge