Name: Period: Date:
Lab: The Mole and Avogadro’s Number
Purpose: To practice using the balance and to practice mole conversions.
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 of # of Moles # of atoms
Mass Substance present in sample
Cup A: Lead
Cup 6: Copper
Cup 7: Iron
Data Table #2
Substance Formula Molar Mass of # of # of # of
Mass Substance Moles molecules atoms in
present in sample sample
Cup B: Water
Cup 1: Sodium
Cup 3: sugar C12H22O11
Cup 4: sodium
A. Fill out the table below:
Substance Formula Representative Given one mole of the Given one mole of the
or Particle, (atom substance, you will substance, you will have . . .
Symbol or molecule) have… of each element
Example: CH4 Molecule 1 mole of CH4 1 mole of Carbon atoms
Methane Molecules 4 moles of Hydrogen atoms
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 1.00 moles of Sodium metal.
2. There are __________ grams in 1.00 moles of Oxygen gas, (formula is O2).
3. There are __________ moles in 110.00 grams of Propane
4. There are __________ moles in 17.20 grams of Silver Nitrate.
5. There are __________ atoms in 156 g of Lead.
6. There are __________ molecules in 128 g of water.
7. There are __________ atoms of Hydrogen in 34 grams of Ammonia.
8. There are __________ grams in 17 millimoles of Cupric Acetate.
9. There are __________ millimoles in 0.105 grams of Manganic Phosphate.