Name:
Period:
Date:
Lab: The Mole and Avogadro’s Number
Purpose: To practice using the balance and to practice mole conversions.
Procedure:
1. Draw the data tables on your own paper
2. Determine the formula of the substance
3. Calculate its molar mass
4. Measure the mass of the sample
5. Complete calculations, showing sample set-ups
6. Answer all questions.
Data Table #1
Substance
Formula
Molar
Mass
Mass of
Substance
# of Moles
present
# of atoms
in sample
Cup A: Lead
Cup 6: Copper
Cup 7: Iron
Cup 8:
Aluminum
Data Table #2
Substance
Formula
Cup B: Water
Cup 1: Sodium
chloride
Cup 3: sugar
Cup 4: sodium
bicarbonate
Cup 5:
magnesium
sulfate
heptahydrate
C12H22O11
Molar
Mass
Mass of
Substance
# of
Moles
present
# of
molecules
in sample
# of
atoms in
sample
Questions:
A. Fill out the table below:
Substance Formula Representative
or
Particle, (atom
Symbol
Formula Unit
or molecule)
Example: CH4
Molecule
Methane
Iron
Given one mole of the
substance, you will
have…
Given one mole of the
substance, you will have . . .
of each element
1 mole of CH4
Molecules
1 mole of Carbon atoms
4 moles of Hydrogen atoms
Water
Carbon
Dioxide
Carbon
Ammonia
B. What is Avogadro’s Number? (include numerical value, as well as description in words)
C. Calculate the indicated conversions below. Use appropriate sig. figures. Must show set-ups.
1. There are __________ grams in 1.50 moles of Sodium metal.
2. There are __________ grams in 3.00 moles of Oxygen gas, (formula is O2).
3. There are __________ moles in 120.00 grams of Propane
4. There are __________ moles in 19.20 grams of Silver Nitrate.
5. There are __________ atoms in 113 g of Lead.
6. There are __________ molecules in 106 g of water.
7. There are __________ atoms of Hydrogen in 37.5 grams of Ammonia.
8. There are __________ grams in 11 millimoles of Cupric Acetate.
9. There are __________ millimoles in 0.135 grams of Manganic Phosphate.