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S'more Stoichiometry Mark as Favorite (13 Favorites)

ACTIVITY in Balancing Equations, Limiting Reactant. Last updated June 04, 2018.

Summary

In this activity, students determine the number of graham crackers and chocolate pieces required to complete a “reaction” with a given quantity of marshmallows (the limiting reactant). They then use the same thought process with a problem involving a real chemical reaction.

Grade Level

High school

Objectives

By the end of this lesson, students should be able to

  • determine mass of product from a given mass of reactant.
  • determine moles of product from a given amount of reactant.
  • write and balance chemical reactions.

Chemistry Topics

This lesson supports students’ understanding of

  • Stoichiometry
  • Balancing equations
  • Limiting reactant

Time

Teacher Preparation: 10 minutes

Lesson: 30-40 minutes

Materials

For each group:

  • Marshmallow
  • Graham cracker
  • Chocolate piece
  • Balance

Safety

  • Food in the lab should be considered a chemical, not for consumption.

Teacher Notes

  • At the beginning of the activity, give each student one marshmallow, graham cracker, and chocolate piece in order to determine their masses. Instruct them to not eat the substances.
  • After students have completed part II of the activity, you can reward students with supplies to make an edible s’mores. Make sure the food items have not been in the lab area. Food should be consumed outside of the lab area.
  • Make sure the students understand that in part I, they are determining how many chocolate pieces and graham crackers needed to use up all of the marshmallows. For example, if they have 10 marshmallows, they can make 10 s’mores, so they would need 20 graham crackers and 30 chocolate pieces (because the chemical formula of a s’more is S2MmOr3).

For the Student

Lesson

Background

“Stoicheion” means element and “metron” means measure. The mass and quantity (mole) relationships among reactants and products in a reaction are found using the process of stoichiometry.

Purpose

To determine the following:

  1. If you are given one bag of large marshmallows, what is the maximum number of S’mores that can be made?
  2. How many boxes of graham crackers and how many chocolate bars are needed to make this many s’mores?

Materials:

  • Marshmallow
  • Graham cracker
  • Chocolate piece
  • Balance

Procedure

PART I: S’MORES REACTIONS

  1. Write a chemical equation using the following symbols (see table):

Substance

Symbol

Unit Mass

Graham Cracker

S

Marshmallow

Mm

Chocolate Pieces

Or

S’more

S2MmOr3

______________ g
  1. Obtain a marshmallow, graham cracker, and chocolate piece. Place each piece of s’more on the balance to determine its unit mass. Record in the table above.
  2. Calculate the unit mass of the S’more (S2MmOr3)below:
  3. a. Write a balanced chemical equation that explains how a s’more is made.
    b. What does the equation tell you?
    c. What do the coefficients represent?
    d. Based on the masses in your table, if you had a bag of marshmallows with a mass of 454 g, how many marshmallows are in the bag?
    e. How many units of graham crackers and chocolate pieces are needed to make the maximum number of s’mores with the number of marshmallows calculated above?
    i. Number of graham crackers needed:
    ii. Number of chocolate pieces needed:
    f. When you go to the store, you cannot determine the exact number of graham crackers or chocolate pieces in a box or bar. The mass is easy to read, however. Using mass values, you can determine how much you need to buy.
    i. If a box of graham crackers has a mass of 254 g, how many boxes do you need to get the number of graham crackers calculated above?
    ii. If one chocolate bar has a mass of 49.5 g, how many bars do you need to buy?

PART II: CHEMICAL REACTIONS

Now you will transfer this process into the language of chemical reactions. If you added a 15.00 g piece of solid Cu to an aqueous solution of silver nitrate, the silver would be replaced in a single replacement reaction forming aqueous copper(II) nitrate and solid silver. How much silver is produced if 15.00 g of Cu is added to the solution of excess silver nitrate? Write and balance the chemical equation:

  1. Convert 15.00g Cu to moles Cu:
  2. Determine moles of Ag produced:
  3. Convert moles Ag to grams of Ag produced:
  4. If silver metal sells for $4.50/ounce, could you get rich from this lab? (How much would it be worth?) Conversion factor: (1 g = 0.0353 oz)