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Drill: Calculate the % composition of each element in Fe 2 (SO 4 ) 3. Molar Conversions. Moles. The standard unit of measure for the amount of a substance in numbers. Dozen. = 12 of anything. Moles. = the amount of a substance that would = its mass in g from the PT. Moles. - PowerPoint PPT Presentation
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Drill: Calculate the % composition of each element in
Fe2(SO4)3
Molar Conversions
Moles•The standard unit of
measure for the amount of a
substance in numbers
Dozen= 12 of anything
Moles= the amount of a
substance that would = its mass in
g from the PT
Moles= 6.022 x 1023
of anything
Molar Conversions• Mass to moles
• Volume of a gas to moles
• Particles to moles
• Volume of a solution to moles
Moles First
Mass to Moles•Use atomic masses from the periodic table
•NaCl = 58.5 g/mole
Gas Volume to Moles•At STP: 22.4 L/mole
•Non-STP: PV = nRTPV
RTn =
Particles to Moles•Use Avogadro’s Number
•6.02 x 1023 atoms, molecules, etc/mole
Soln Volume to Moles
•Multiply molarity times volume
•n = M x V
Solution Measures•Molarity (M) = the number of moles of solute per liter of solution
•Others later
Calculate the atomic mass of the element made up of the
following isotopes:99.50 % H-10.30 % H-20.20 % H-3
Calculate the atomic mass of the element made up of the
following isotopes:5.0 % Pu-242, 5.0 % Pu-243
80.0 % Pu-244, & 10.0 % Pu-245
•Convert 7.0 g of silicon to
moles
Convert 250 g of CaCO3
to moles
Convert 3.0 moles of helium
to grams
Convert 5.6 L of oxygen gas at STP to moles
Convert 0.50 moles of helium
to volume at STP
Convert: 2.0 x 1024 atoms
He to moles
Convert 3.0 moles of glucose
to molecules
Convert 250 mL of 0.10 M HCl
to moles
Drill: Determine the volume
required to make 60.0 g NaOH into a 0.75 M solution
Convert 6.8 g NH3 to volume
at STP
Convert 3.0 x 1025 molecules of CO2
to mass in kg
Calculate the number of oxygen atoms in 32 g of
Fe2O3
Calculate the number of atoms
in 16 ng of Fe2(SO4)3
Drill: Calculate the mass of solute
required to make 40.0 mL of
0.25 M Pb(NO3)2
Test Review on Nomenclature,
Molar conversions, & % Composition.
Calculate the % composition of each element in
Pb(NO3)2
Calculate the empirical formula of
a substance comtaining 62.7 %
Po, 28.8 % O, & 8.4 % N.
Calculate the molecular formula of a substance with an empirical formula of NH2 & a molecular mass of 32 g/mole.
Name each of the following:
•SeO MgS
•PbO2 Cl2O
•KNO3 ScCl3
Derive formulas for each:
•Cesium oxide
•Barium chloride
•Calcium phosphate
•Manganese(II) chlorate
Name each of the following:
NH4Cl BaSO4
KC2H3O2 K2HPO3
KNO3 CuBrO
Li2CO3 MgC2O4
Name each of the following:
HCl H2SO4
H2S H3PO3
HNO3 HBrO
H2CO3 HBrO4
Calculate the number of
hydrogen atoms in 1.8 kg of PH5.
Calculate the volume at STP of
6.0 ng of NO.
Calculate the mass of KBr required to make 250 mL of a 0.40 M solution.
Chapter 3 General
•Define all the Key Terms on page 74
Atomic Mass
•Work problems:
1 - 9
on page 75
Avogadro’s Num.
•Work problems:
11 - 18
on page 75
Molar Conversions
•Work problems:
18 - 26
on page 75 & 76
% Composition
•Work problems:
27 - 34
on page 76
Empirical Formula
•Work problems:
35 - 46
on page 76 & 77
Balancing Rxns
•Work problems:
49 & 54
on page 77
Stoichiometry
•Work problems:
55 & 64
on page 77 & 78
Limiting Reactant
•Work problems:
65 & 74
on page 78 & 79