1. Mole-Mole Conversions Mass to Mass Calculations
Day 1: Intro & How to

2. Evaluation/Assessment:
Objective:
Today I will be able to:
Construct mol to mol ratios in order to convert from the mass of a reactant to the mass of a product
Evaluation/Assessment:
Informal Assessment – Monitoring group interactions as the students complete the mass-mass calculations
Formal Assessment – Analyzing student responses to the mass-mass practice and exit ticket
Common Core Connection
Make sense of problem and persevere in solving them
Model with mathematics
Use appropriate tools strategically
Look for and express regularity in repeated reasoning

3. Lesson Sequence Evaluate: Warm – Up Evaluate: Review HW
Explain: Stoichiometry – Mass-Mass Calculations
Elaborate: Mass-Mass Calculations Practice
Evaluate: Exit Ticket

4. Warm - Up Determine the type of representative particle: a) Br2
(Hint: atom, formula unit, molecule)
a) Br2
b) CaSO4
c) NH4Cl
d) Hg
e) P2O5
f) Al2O3

5. Objective Today I will be able to:
Construct mol to mol ratios in order to convert from the mass of a reactant to the mass of a product

6. Homework
Finish Mass-Mass Calculations

7. Agenda Warm-Up Review HW Mass-Mass Calculation Notes
Mass-Mass Calculation Practice
Exit Ticket

8. What questions do you have about the practice problems from yesterday?
Review HW
What questions do you have about the practice problems from yesterday?

9. Stoichiometry: Mass - Mass Calculations

10. What is Stoichiometry?
The study of quantitative (measurable) relationships that exist in chemical formulas and chemical reactions

11. Mol-Mol Ratios
To convert from mass of a reactant to mass of a product we need to use the mol ratio
Mol ratios are determined using the balanced chemical equations
Example: 2 H2 + O2  2H2O
Example Ratios:

12. Mass-Mass Problems
You are given the mass of one substance and are asked to find the mass of another substance involved in the same reaction
Steps to solving mass-mass problems
Mass of given  moles of given  moles of unknown  mass of unknown
(Use Mol Road Map)

13. Mass-Mass Problems Example: 2 Al + Fe2O3  2 Fe + Al2O3
What mass of iron (III) oxide was supplied if 2.3 g of aluminum oxide was produced in the reaction?
1 mol Fe2O3
1 mol Al2O3
160 g Fe2O3
1 mol Fe2O3
2.3 g Al2O3 1
1 mol Al2O3
102 g Al2O3 x x x =
3.6 g Fe2O3

14. Mass-Mass Problems
Determine the mass of sodium hydroxide produced when .25 g of Na reacts with water.
2 Na + 2 H2O  2 NaOH + H2
.25 g Na 1
1 mol Na
23 g Na
2 mol NaOH
2 mol Na
40 g NaOH
1 mol NaOH x x x =
.43 g NaOH

15. Exit Ticket Predict the products of the equation and then balance:
Mg + HCl 
What is the mol ratio between HCl and MgCl2?
If you have 4.0 mol of HCl how many mol of MgCl2 are present?