Period: ______ Name: ________________________________________
What’s in a Mole?
Part 1: Molar Mass
Use a periodic table to complete the molar mass section in the table. The last column will be completed in Part 2.
Chemical Formula
Molar Mass g/mol
Mole of what?
Equivalent to:
Cu (s)
63.55 g/mol
of Cu atoms
50ft of 20-gauge copper wire
O2 (g)
32.00g/mol
of oxygen molecules
22.4L of oxygen gas at STP
Ni (s)
Al (s)
H2O (l)
He (g)
22.4L of helium gas at STP
NaCl (s)
Hg (l)
14.7mL of mercury
Fe (s)
C12H22O11 (s)
0.75lb of sugar
Questions:
1. One mole contains how many particles?
2. How many copper atoms are in 63.55g of copper?
3. Copper has a larger molar mass than aluminum. Explain what this means.
4. Which contains more moles, 1.0g Al(s) or 1.0g Hg (l)? Explain your thinking using unit analysis as proof.
5. Explain step wise how to determine the molar mass of sugar (C12H22O11). Show your work.