Name: Click here to enter text.
Basic Stoichiometry PhET Lab
Let's make some sandwiches!
Introduction:
When we bake/cook something, we use a specific amount of each ingredient.
Imagine if you made a batch of cookies and used way too many eggs, or not
enough sugar. In chemistry, reactions proceed with very specific recipes. The
study of these recipes is stoichiometry. When the reactants are present in the
correct amounts, the reaction will produce products. What happens if there are
more or less of some of the reactants present?
Vocabulary: Before you begin, please define the following:
Limiting Reactant:
Click here to enter text.
Excess Reactant: Click here to enter text. Synthesis Reaction: Click here to enter text. Combustion Reaction: Click here to enter text. Mole Ratio: Click here to enter text. Diatomic Molecule: Click here to enter text. Mole: Click here to enter text. Hydrocarbon: Click here to enter text. Procedure: PhET Simulations Play with the Sims Chemistry Reactants, Products, and Leftovers
If a yellow bar drops down in your browser, click on it and select "Allow Blocked Content"
Part 1: Making Sandviches:
1. The
is a simulation of a two-reactant synthesis reaction. In this case,
one reactant will be limiting, while the other will be in excess. Take some time and familiarize
yourself with the simulation.
2. Set the reaction to a simple mole ratio of 2:1:1 C. Bires, revised 11/2013 Simulations at http://phet.colorado.edu/ Adapted from a lab exercise created by Chris Bires
https://phet.colorado.edu/en/contributions/view/3786 3. Complete the table below while making tasty cheese sandwiches:
Bread Used
Cheese Used
Sandwiches
Excess Bread
Made
5 slices
5 slices
Click here to enter
Click here to
text.
enter text.
4 slices
3slices
Click here to enter
Click here to
text.
enter text.
Click here to
Click here to
2 sandwiches
1 slice
enter text.
enter text.
6 slices
Click here to
3 sandwiches
Click here to
enter text.
enter text. Excess Cheese
Click here to
enter text.
Click here to
enter text.
0 slices
4 slices Part 2: Real Chemical Reactions:
4. Now let's work with real chemical reaction, one that creates a very entertaining
BOOM! What is the mole ratio for the reaction of hydrogen and oxygen to produce water?
Click here to enter text.H2
+ Click here to enter text. O2
──────────────────
Click here to enter text.H2O
5. Complete the table below while making water H2O from hydrogen H2 and oxygen O2:
Hydrogen Molecules Oxygen Molecules
Water Molecules
Excess H2
Excess O2
H2
O2
H2O
4 molecules
4 molecules
Click here to enter
Click here
Click here to
text.
to enter
enter text.
text.
7 molecules
6 molecules
Click here to enter
Click here
Click here to
text.
to enter
enter text.
text.
Click here to enter
Click here to enter
4 molecules
0
0 molecules
text.
text.
molecules
9 moles
8 moles
Click here to enter
Click here Click here to
text.
to enter
enter text. text. C. Bires, revised 11/2013 Simulations at http://phet.colorado.edu/ Adapted from a lab exercise created by Chris Bires
https://phet.colorado.edu/en/contributions/view/3786 Hydrogen Molecules
H2
Click here to enter
text.
4.0 moles Oxygen Molecules
O2
Click here to enter
text.
2.5 moles 1.5 moles Click here to enter
text. Water Molecules
H2O
4 moles Excess H2 Excess O2 1 moles 0 moles Click here to enter
text. Click here
to enter
text.
0 moles Click here to
enter text. 1.5 moles 0 moles 6. Notice that the labels changed from molecules to moles. This does not change the mole ratio, as
a mole is simply a large number of molecules.
How many molecules is a mole? Click here to enter text.
7. Now try producing ammonia, a very important chemical in industry and farming.
What is the mole ratio for the production of ammonia? __ N 2 __ H 2 __ NH 3 Click here to enter text.
8. Complete the table below:
Moles N2
Moles H2 Moles NH3 Excess N2 Excess H2 Click here
to enter
text.
Click here
to enter
text.
2 moles Click here to
enter text. Click here
to enter
text. Click here to
enter text. 3 moles 6 moles Click here to enter
text. 6 moles 3 moles Click here to enter
text. Click here to enter
text.
1.5 moles Click here to enter
text.
4.0 moles 4 moles
Click here to enter
text. Click here to
enter text.
0 moles 9. Combustion of hydrocarbons like methane CH4 produces two products, water and carbon dioxide
CO2.
What is the mole ratio for the combustion of methane? __ CH 4 __ O2 __ CO2 __ H 2 O Click here to enter text. C. Bires, revised 11/2013 Simulations at http://phet.colorado.edu/ Adapted from a lab exercise created by Chris Bires
https://phet.colorado.edu/en/contributions/view/3786 10. Complete the table below: WATCH FOR FRACTIONS
mol CH4
mol O2
mol CO2
mol H2O
Excess mol CH4
4 mol 4 mol 3 mol 6 mol Click here
to enter
text. Click
here to
enter
text.
Click
here to
enter
text. Click here
to enter
text. Excess mol O2 Click here
to enter
text.
Click here
to enter
text.
2 mol Click here
to enter
text.
Click here
to enter
text.
4 mol Click here to enter
text. Click here to enter
text. Click here to enter
text. Click here to enter
text. Click here to enter
text. Click here to enter
text. 3 mol Click here
to enter
text. Click here to enter
text. Click here to enter
text. Basic Stoichiometry Post-Lab Exercises
Complete each exercise. Remember to use proper units and labels.
1. For the reaction __ N 2 __ O2 __ NO2 determine the correct lowest mole ratio.
Click here to enter text. 2. For the reaction __ SO2 __ O2 __ SO3 determine the correct lowest mole ratio.
Click here to enter text. 3. For the reaction P4 6Cl 2 4 PCl3 , determine how many moles of chlorine Cl2 would be needed to react with 3 moles of phosphorus P4 to entirely use up all the phosphorus.
4) Click here to enter text.
4.
If 5 moles of P4 reacted with 22 moles Cl2 according to the above reaction, determine:
a) How many moles PCl3 are produced
a) Click here to enter text.
b) How many moles of P4 are left in excess after the reaction (if any) b) Click here to enter text. c) How many moles of Cl2 are left in excess after the reaction (if any) c) Click here to enter text. C. Bires, revised 11/2013 Simulations at http://phet.colorado.edu/ Adapted from a lab exercise created by Chris Bires
https://phet.colorado.edu/en/contributions/view/3786 In reality, reactants don't have to react in perfect whole-numbers of moles. In a two-reactant synthesis
reaction, usually one reactant gets entirely used up (and determines how much product is
made), even if that means using fractions of a mole of reactant. For instance, when solid, metallic
aluminum Al and red, liquid bromine Br2 are brought together, they make a white solid according to the
reaction 2 Al 3Br2 2 AlBr3 . If 5.0 moles of aluminum Al was reacted with 10 moles bromine Br2, all five moles of aluminum would react, with only 7.5 moles bromine. (2:3 mole ratio) This would
produce only 5.0 moles of AlBr3, leaving 2.5 moles of excess Br2 behind. 5.
Now assume 3 moles Al and 4 moles Br2 react
a) Which chemical is the limiting reactant? a) Click here to enter text. b) Which chemical must be the excess reactant? b) Click here to enter text. c) How much (in moles) AlBr3 gets produced?
Click to show work here. c) Click here to enter text. d) If all the limiting reactant gets used up, how much of the excess reactant is left?
d) Click here to enter text.
Click to show work here. 6. What is the maximum amount (in moles) of NaCl that can be produced from 4.5 moles of Na and 3.5 moles of Cl2 according to the reaction __ Na __ Cl 2 __ NaCl (left for you to balance).
7) Click here to enter text. Click to show work here. C. Bires, revised 11/2013 Simulations at http://phet.colorado.edu/ Adapted from a lab exercise created by Chris Bires
https://phet.colorado.edu/en/contributions/view/3786

 

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