1. Mole and Stoichiometry Mini-Lab
Procedures
Record mass in grams of aluminum soda can.
Record volume of water in graduated cylinder.
Calculate and record the mass of water in graduated cylinder.
Show work for conversion using the density of water (1.00 g/mL) as the conversion factor.
Data Table
Substance
Mass (g)
Volume (mL)
Aluminum
Water

2. Your Name U7-7 Mole and Stoichiometry Mini-Lab 01/28/2013
Substance
Mass (g)
Volume (mL)
Aluminum
13.3 g
Water
22.8 g
22.8 mL
22.8 mL H2O
1.00 g H2O
1 mL H2O
g H2O =
= 22.8 g H2O

3. Mole and Stoichiometry Mini-Lab
Calculations: Show ALL work (bridge/grid).
The GIVEN for calculations #1 and #2 should be measurements, not results from a previous calculations.
How many moles of aluminum are in the soda can?
How many atoms of aluminum are in the soda can?
For an experiment, 2.5 moles of aluminum is needed. Since there is no measuring tool for moles, how would a researcher measure out this much aluminum?
Respond to question in complete sentence and show work for necessary calculation.
UNKNOWN: mol Al GIVEN: g Al (data table)
UNKNOWN: atoms Al GIVEN: g Al (data table)
UNKNOWN: g Al GIVEN: 2.50 mol Al

4. Mole and Stoichiometry Mini-Lab
Calculations: Show ALL work (bridge/grid).
The GIVEN for calculations #4 and #5 should be measurements, not results from previous calculations.
How many moles of water are in the graduated cylinder?
How many molecules of water are in the graduated cylinder?
For an experiment, 4.75 moles of water are needed.
How many grams of water are needed?
How many millilters of water would this be?
UNKNOWN: mol H2O GIVEN: g H2O (data table)
UNKNOWN: molecules H2O
GIVEN: g H2O (data table)
UNKNOWN: g H2O GIVEN: 4.75 mol H2O
UNKNOWN: mL H2O GIVEN: 4.75 mol H2O

5. Mole and Stoichiometry Mini-Lab
Write and balance the equation for the reaction between aluminum and water to produce aluminum oxide and hydrogen gas.
Using the moles of the aluminum can in #1 as the GIVEN, how many moles of hydrogen gas can be produced? Assume water is available in excess.
Using the moles of water from #4 as the GIVEN with aluminum in excess, calculate the number of moles of aluminum oxide that can be produced.
2 Al H2O → Al2O H2
Al + H2O → Al2O3 + H2
UNKNOWN: mol H2 GIVEN: mol Al (answer to #1)
UNKNOWN: mol Al2O3 GIVEN: mol H2O (answer to #4)

6. Mole and Stoichiometry Mini-Lab
Conclusion
Part 1: Write a dialogue between You the Expert and You the Novice about the calculation for #8.
You the Expert are explaining how to calculate the answer to the problem and why each step is necessary.
You the Novice are asking questions about the process and making comments about your level of understanding.
Part 2: In a well-developed paragraph, explain the procedures that were necessary to complete the calculation in #9.
PAST TENSE (what was done and why)
Write objectively (no 1st or 2nd person voice, no personal pronouns)