Mole Lab
Background: One mole of anything consists of 6.02 x 1023 units of that substance. The Periodic Table
shows the average atomic mass of 1 mole of each element. The mass of one mole is called the
substance’s molar mass. The unit for molar mass is grams per mole (g/mol).
Purpose: The purpose of this lab is to gain a better understanding of the mole.
In this lab you will find the mass of one mole of 3 metal samples and identify the metal by its molar
mass. The metal samples are labeled A, B, and C. Then you will calculate the number of moles in a
sample of Ammonium Chloride, Sodium Chloride, and Sucrose (C12H22O11).
Procedure Part 1: Metal Samples
1. Write a brief qualitative description of each metal sample.
2. Find and record the mass of each 1 mole metal sample + container provided.
3. Calculate the mass of the sample.
4. Using your periodic table, your observation, the mass of each sample, and the fact that each
sample is one mole, determine the identity of each metal sample.
5. Identify the number of atoms found in each 1 mole sample.
Procedure Part 2: Solid Compounds
1. Record the formulas for the solid compounds. (The formula for sucrose is given in the
background information.)
2. Write a brief qualitative description of each metal sample.
3. Find and record the mass of each sample + container.
4. Calculate the mass of the sample.
5. Calculate the molar mass of each substance using the periodic table.
6. Calculate the number of moles and number of particles in each sample. Show your work in
the space provided using factor-label method.
Analysis and Calculations
Answer all of the analysis questions and show your work for the calculations.
Mole Lab
Name ________________________
Date _________________ Per ___
Data Table 1 – Metal Samples
Sample
A
B
C
4.54g
5.09g
4.60g
1 mole
1 mole
1 mole
Physical
Appearance
Mass of
sample +
weigh boat
(g)
Mass of
empty
weigh boat
(g)
Mass of
sample
(g)
Identity of
Metal
# of moles
# of atoms
Analysis
1. Explain why your lab values were not exactly the same as the value form the periodic table.
2. Why was the mass of each metal sample different even though each sample was one mole?
3. Why does a similar mass of substances not necessarily mean a similar number of moles of a substance?
4. Why do you think chemists use the mole instead of referring to the number of molecules, atoms, or units of
a substance?
Mole Lab – data page2
Data Table 2 – Solid Compounds
Name ________________________
Sample
1
2
3
Substance
Ammonium Chloride
Sodium Chloride
Sucrose
8.186g
8.173g
8.410g
Formula
Physical
Appearance
Mass of
sample +
container
(g)
Mass of
empty
container
(g)
Mass of
sample
(g)
Actual
Molar Mass
# of
moles
# of
particles
Conclusion:
1. How many grams of sand (SiO2) would need to be weighed out to equal 0.3 moles?
2. How many grams would be weighed out to equal 6.02 x 1023 molecules of water?