INDIVIDUAL BRAINSTORM: Silently, make a list of the best places to get a burger. (1 minute) GROUP BRAINSTORM: Rank the top three places to get a burger.

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Presentation transcript:

INDIVIDUAL BRAINSTORM: Silently, make a list of the best places to get a burger. (1 minute) GROUP BRAINSTORM: Rank the top three places to get a burger. What made the burger so great? (2 minutes)

A burger recipe might look like this: 1 Bu + 2 Hb + 1 Ch + 4 Ba 1 Ub As a group, develop your ultimate burger recipe and write it as an equation. Here are the available ingredients: Buns Hamburger (patties) Bacon (strips) Cheese (slices) Lettuce (leaves) Tomato (slices) Onion (slices) Pickle (slices) Mustard (squirts) Ketchup (squirts)

Using the ingredients handout from Ms. Brown, answer these questions: 1. How many complete burgers can you make? 2. Which ingredient(s) is/are completely used up? 3. How much of each leftover ingredient remains unused? 4. List and explain the steps that your group used to answer the questions above.

Now, write three (3) problems and their solutions based on your burger recipe. Example: If Annie has 18 strips of bacon, how many burger patties does she need to completely use up her bacon? 1 Bu + 2 Hb + 1 Ch + 4 Ba 1 Ub 18 Ba2 Hb = 9.0 Hb 4 Ba

Your ultimate burger recipe Your answers to the 4 questions Your three problems with solutions Your group answers to these reflection questions: 1. How well did your group come to consensus today? Explain. 2. What do you think that this activity has to do with chemistry content? 3. Are you hungry right now?

[stoy-key-AH-meh-tree]

DEFINITION: calculation of quantities in reactions KEY STEP: mole ratio from balanced equation So, to do stoichiometry, you need a balanced equation!

N2N2 +3 H 2 2 NH 3 1 molecule N 2 +3 molecules H 2 2 molecules NH 3 1 mole N 2 +3 moles H 2 2 moles NH g N 2 + 3(2.016) g H 2 = g H 2 2( ) g NH 3 = g NH 3 particles moles mass

4 Fe+3 O 2 2 Fe 2 O particles moles mass

Ratio between the numbers of moles of any two substances in a balanced chemical equation Example: 2 KClO 3 2 KCl + 3 O 2

How many moles of oxygen gas can be produced by the reaction of 5.85 moles of potassium chlorate? 2 KClO 3 2 KCl + 3 O 2

How many liters of oxygen gas at STP can be produced by the reaction of 47.9 grams of potassium chlorate? 2 KClO 3 2 KCl + 3 O 2

rep. particles Arep. particles B grams Amole A use mole ratio! mole Bgrams B liters Aliters B

How many liters of oxygen gas at STP can be produced by the reaction of 47.9 grams of potassium chlorate? 2 KClO 3 2 KCl + 3 O 2