Download Ministry Strand: Quantities in Chemical Reactions Teacher

Ministry Strand: Quantities in Chemical Reactions
Associate Teacher: Marcel Dufresne
Unit Day #: 13
Teacher Candidate: Jake Morra
Activity: Stoichiometry (Part 3)
Time: 70 minutes
Specific Expectation:
D2.1 - use appropriate terminology related to quantities in chemical reactions, including, but not limited to:
stoichiometry, percentage yield, limiting reagent, mole, and atomic mass
D 2.5 - calculate the corresponding mass, or quantity in moles or molecules, for any given reactant or
product in a balanced chemical equation as well as for any other reactant or product in the chemical reaction
D 3.4 - explain the quantitative relationships expressed in a balanced chemical equation, using appropriate
units of measure (e.g., moles, grams, atoms, ions, molecules)
Previous
Warm-Up Activity
Materials Needed
Homework
From textbook:
- pop bottle demonstration
- 3 pop bottles
p.237 #1,2, p. 238
- SMART Board and SMART Notebook 13
#4,5,7, p. 240 #9
- Handouts (see attached)
- SCH3U1 Textbook
Activity Descriptions:
- To begin lesson, instructor will show 4 diagrams on SMART Board:
-
Ask which .5 L bottle would produce a “pop” sound first if it was heated from the outside, given
that hydrogen gas only produces the “pop” sound when it undergoes combustion (students have
seen this reaction in their handout) (http://www.youtube.com/watch?v=ZoFrfz49pe0)
After vetting for answers, write the equation _H2 + O2 -> _H2O (have students fill in the
coefficients (2 and 2).
In pairs, have students use stoichiometry to determine which bottle will make the pop sound first.
Answer: bottle 3 is the only bottle that will fully use all of the O2 and H2 to react in a combustion
reaction (having .5/3 L of O2 and 2*.5/3 L H2, the optimal ratio for the combustion reaction)
Instructor will then do 3 worked examples (1 with mass, 1 with volume, 1 with # particles)
Students will use the rest of this lesson to review for the quiz tomorrow (stoichiometry).
For consolidation, a specific textbook problem will be taken up in class (solution attached)
Consolidation Activity
Assessment and Evaluation
- Instructor will take up the
- Instructor will assess
first handout problem
some student
understanding during
- An outline of quiz items will
pair-work and review
be written on board.
Homework
- Review (or complete)
yesterday’s homework
(has mole, volume,
mass, and particle
stoichiometry questions)
, review day 2 handouts
Stoichiometry, Day 3 – Quiz Outline and In-Class-Examples
Items for Quiz:
1) balancing chemical equations (finding species coefficients)
2) finding moles of a species using mole ratios
3) finding moles, given mass, volume, or # particles
4) finding mass, volume, or #particles using moles
Note: any questions will be essentially taken from homework or class examples (with numbers changed)
Class examples:
1) The Haber process combines hydrogen (H2) with nitrogen (N2) to produce ammonia (NH3). At STP, how
many moles of ammonia can you produce, given that you have 44.8 L of H2?
N2(g) +3H2(g) → 2NH3(g)
2) Calcium carbonate (CaCO3) produces carbon dioxide and calcium oxide at high temperatures:
CaCO3(s)  CO2(g) + CaO(s)
How many grams of calcium carbonate would you need to make 3.45 L of carbon dioxide (assume STP)?
3) Use the equation below:
Pb(SO4)2 + 4 LiNO3  Pb(NO3)4 + 2 Li2SO4
How many grams of LiNO3 (lithium nitrate) are required to produce 250 grams of Li2SO4 (lithium sulfate),
given a sufficient amount of lead (IV) sulfate?
Consolidation example:
H2 gas (hydrogen gas) can be produced by reacting methane (CH4) with high temperature steam. How many
particles of H2 are produced when 158 g of methane reacts with steam (Note: 1 mol = 6.02× 1023 particles)?
CH4(g) + H2O(g) → CO(g) + 3 H2(g)
*USE THE 5 STEPS
1. Given: have 158 g of CH4
Find: want moles of H2
2. convert g of CH4 to moles:
3.
1 mole of CH4: 3 moles of H2
1:3 mole ratio
4.
9.875 moles CH4 produces
moles H2
5.
H2