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Moles: Measuring Matter
A UNIT OF MEASURE!!!A UNIT OF MEASURE!!!
1 mole = 6.02 x 1023 representative particles– atoms, molecules, formula units, ions– Also called Avogadro's number
Moles
1 mole = 6.02 x 1023 particles 1 mole is also equal to the molar masmolar mass of a substance molar mass = atomic mass with the units g/mol
*g/mol is the same as atomic mass except atomic mass has the units of amu
Molar mass of compoundsMolar mass of compounds – add up parts– Find the molar mass of KK22CrOCrO44
Mole Conversions
particles to molesparticles to moles
# particles 1 mole
6.02 x 1023 particles moles to particlesmoles to particles
# moles 6.02 x 1023 particles
1 mole moles to mass (g)moles to mass (g)
moles molar mass =
1 mole
Mole Conversions
Mass (g) to molesMass (g) to moles
mass 1 mol =
molar mass Mass (g) to particlesMass (g) to particles
mass 1 mol 6.02 x 1023 particles
molar mass 1 mol particles to mass (g)particles to mass (g)
particles 1 mol molar mass
6.02 x 1023 particles 1 mol
MOLES to Particles
Converting moles to particles– Conversion Factors
# moles x 6.02 x 1023 particles
1 molConvert 3.5 moles sucrose to molecules
Moles continued
Converting particles to moles
# particles x 1 mole =
6.02 x 1023 particlesCalculate the # moles in 4.50 x 10Calculate the # moles in 4.50 x 102424 atoms Zn atoms Zn
Moles: Mass and the Mole
Moles to mass:Moles to mass:
# moles x # grams
1 mol– How many grams are in 3.00 mol Mn?
Moles -2: Mass and the Mole
atoms to mass:# particles x 1 mol x # grams
6.02 x 1023 particles 1 mol
– How much mass is in 5.50 x 10How much mass is in 5.50 x 102222 atoms of atoms of helium?helium?
mass to atoms:mass x 1 mol x 6.02 x 1023atoms
#grams 1 mol– How many atoms of gold in 25.0 g?How many atoms of gold in 25.0 g?
Moles -4: Empirical and Molecular Formulas
percent composition
mass of element x 100 = % by mass
mass of compound
• percent always adds up to 100– Find % of H and O in water
Moles -4 continued
Empirical formula – smallest whole # mole ratio of the elements
* May or may not be actual molecular formula– To get:
1. Change g to mol
2. Get mole ratio
3. The ratios are the subscripts*If you are given % composition: assume % is grams
Find the empirical formula of a sample with 40.05 g S and 59.95 g O.
Moles -4 continued
Molecular formula – specific # of atoms of each element in compound
experimentally determined molar mass = n
mass of empirical formulamultiply n by empirical formula subscripts
molecular formula = (empirical formula)n
Problem: The empirical formula of a substance is CH. The molecular mass of the compound is 78 amu. What is the molecular formula of the compound?
EMPIRICAL & MOLECULAR FORMULA PRACTICE
– Chemical analysis indicates a sample is composed of 40.68% C, 5.08% H and 54.24% O and has a molar mass of 118.1 g/mol. Determine the empirical and molecular formulas of succinic acid
Moles: Moles of Compounds
YOU can find moles of a part of a compound– How many moles of F are in 5.50 moles
CCl2F2?
* Get ratio from formula.– Determine the number of moles of Al ions in
1.25 mol Al2O3
Moles -5: The formula for a Hydrate
Hydrate – compound with a specific # of water molecules bound to its atoms
Methane Hydrate
Naming Hydrates
Naming:Naming:– name salt • prefix hydrate
CaCl2•2H2Ocalcium chloride dihydrate
– Prefixes are the same as those used for covalent compounds
– Anhydrous – without water used to store water or as drying agents
– Used to store solar energy i.e. sodium sulfate decahydrate