Name _________________________________ Period ______ Pg # __________
Types of Chemical Reactions Lab
Objectives:
1) To observe chemical reactions and record evidence that a new product formed.
2) To write a balanced chemical equation for each reaction observed.
3) To predict products for the different types of reactions.
4) To classify each reaction observed as a synthesis, decomposition, single replacement, double
replacement or combustion reaction.
Safety:
1) Wear goggles and aprons for the entire portion of the lab.
2) Tie back long hair and secure loose articles of clothing/ID’s.
3) If any chemical spills on your hands during a reaction, wash IMMEDIATELY with soap and running
water. If you spill acid on your skin, wash and rinse for 3 minutes. If you splash acid in your eye,
flush eyes with water for 20 minutes at the eyewash station or nearest sink.
Reaction 1: Methane Bubbles (teacher demo)
Evidence of a
chemical reaction
1. Write the complete and balanced equation for this reaction (don’t forget your diatomic elements or HOFBrINCl):
Words:
Methane
Formulas:
_______ +
+
oxygen

______

________________ +
__________
+
_________________
_______________
2. What type of reaction was demonstrated above? (circle correct answer)
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
3. How will you recognize this type of reaction?_____ ______________________________________________________
4. Predict products and balance the following reaction:
C2 H6 +
O2

5. Using the equation above, if 1.25 grams of C2H6 react with 0.25 grams of oxygen, 0.50 grams of water get produced.
How much carbon dioxide is also produced in this reaction? (HINT: SOLVE FOR x!)
6. Describe in your own words what is meant by the “Law of Conservation of Mass.” __________________________
________________________________________________________________________________________________
Reaction 2:
1. Light your Bunsen burner.
2. Observe your magnesium ribbon before the reaction. Observe any observations.
3. Take a 1-inch piece of magnesium ribbon and hold it in the flame. CAUTION: NEVER LOOK INTO A BRIGHT LIGHT. IT
COULD CAUSE RETINAL DAMAGE.
4. Look at the ribbon now! Notice how it changed appearance. Note observations.
5. Clean up counter for the next group.
Observations of magnesium
before reaction
Observations of product
after reaction
6. Write the complete and balanced equation for the reaction observed. Use the data collected to predict the correct
product:
Words:
Magnesium
+ oxygen (in air) 
_________________________
Formulas:
___________
+
_______

_______________
7. What type of reaction was demonstrated above? (circle correct answer)
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
8. How will you recognize this type of reaction?___________________________________________________________
9. Predict products and balance the following reaction:
Al +
S 
Reaction 3:
1. Fill a plastic tub about ½ full of water. Place a large test tube into the water, fill it with water, and invert it
into the tub of water so now it’s upside down. Try to minimize the amount
of air trapped at the top of the inverted test tube.
2. Run the rubber tube inside the mouth of the inverted test tube. See diagram.
3. Pour in 15 mL of HCl into the tube mounted on the ring stand.
Tub
4. Add in a few pieces of zinc metal, and stopper the large test tube tightly.
Note observations about what happens below.
5. Allow the collecting test tube under water to completely fill with gas.
6. Keeping the tube inverted, remove the tube from the water and place it
mouth down onto the laboratory bench. The gas will not escape.
7. Light a match and light a wooden splint, lift the test tube and place the
lighted splint into the mouth of the test tube. The quicker you get the
flame under the tube, the better it works. A whistling sound should be
heard. Do not drop the test tube, you will be fine. Note what happened below.
8. Any solids left over should be thrown away in the trash can. The liquids can be washed down the drain with
lots of water. CAREFUL! The reaction test tube will be warm.
Evidence of a chemical
reaction
Observations with flame
9. Write the complete and balanced equation for the reaction observed. Use the data collected to predict the correct
product:
Words:
Hydrochloric acid + zinc 
____________________ + ______________________
Formulas:
___________
+
_______ 
_______________
+
___________________
10. Looking at the products formed, which product above was the one that reacted with the flame? ________________
11. What type of reaction was demonstrated above? (circle correct answer)
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
12. How will you recognize this type of reaction?__________________________________________________________
13. Predict products and balance the following reaction:
Al
+
H2SO4

14. Which of the following reactions is obeying the Law of Conservation of Mass?
a.
b.
c.
d.
4NaF + 4 H2SO4 
4 HF + Na2SO4
Mg + O2

2 MgO
CaF2 + 2 Fe
 2FeF
+ 2Ca
2Al2O3
 4Al +
3O2
Reaction 4:
1. Place about 30 drops of silver nitrate solution into a test tube. Place the test tube in the test tube rack.
2. Place about 30 drops of sodium chloride solution into the same test tube. Record your results.
Observations of
reactants
Observations of
products
3. Write the complete and balanced equation for the reaction observed. Use the data collected to predict the correct
product:
Words:
silver nitrate
Formulas:
___________
+
sodium chloride
+

____________________ + ______________________
___________ 
_______________
+
___________________
4. What do you call a solid formed by two aqueous solutions? _______________________________________________
5. What type of reaction was demonstrated above? (circle correct answer)
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
6. How will you recognize this type of reaction?___________________________________________________________
7. Predict products and balance the following reaction:
Na2SO4 +
KCl

Reaction 5:
Background: We have prepared an electrolysis solution for you consisting of water and a little dash of salt to act as a
conductor. Remember that water is NOT conductive since it consists of two nonmetals (and covalent!). The universal
indicator is a chemical that tests the pH levels of a chemical much like litmus paper, but a lot more specific. The
universal indicator does NOT take part in the reaction and is really just for fun! Not really… the universal indicator is
really to test for the evidence of the formation of gases produced. The negative electrode will produce hydrogen gas.
The positive electrode will produce oxygen gas. Colors like pink, orange and yellow will indicate that oxygen has been
released. Colors like blue-green, blue and purple will indicate that hydrogen has been released.
1. Pour electrolysis solution into a Petri dish until it is about ½ full. Add 7 drops of universal indicator to your dish.
Place your Petri dish on your white paper.
2. Attach one alligator clip to the left edge of the dish. Do the same thing with a second alligator clip on the right side of
the dish.
3. The ends of the clips should be covered by the green solution.
4. Attach your other ends of your alligator clips to the two opposite prongs of the battery.
5. Let the reaction proceed for 5 minutes and note the changing colors over time.
Time
1 minute
2 minutes
3 minutes
4 minutes
5 minutes
Observations that a chemical reaction
is taking place:
Color on (+) electrode
Color on (-) electrode
6. Which electrode produced more bubbles? What do you think that implies about the number of moles being
produced at this electrode? ___________________________________________________________________________
7. Which electrode produced oxygen gas? _____________________________________________________________
8. Which electrode produced hydrogen gas? ___________________________________________________________
9. Write the complete and balanced equation for the reaction observed.
Words:
Water
Formula:

_____________
+
_______________
_____________ 
___________
+
___________
10. What type of reaction was demonstrated above?
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
11. How will you remember this type of reaction? ________________________________________________________
12. Predict products and balance the following reaction:
Al2S3

Demonstrations 6 – 10:
6. Magnesium and water 
_______ +
_________
_____________________

______________
Evidence of a chemical reaction: ________________________________________________________________
7. Calcium and water  ______________________________
______ + __________  ________________
Evidence of a chemical reaction: ________________________________________________________________
8. Sodium and water  _______________________________
_______ + ________  _________________
Evidence of a chemical reaction: ________________________________________________________________
9. Potassium and water  _____________________________
_______ + ________ 
__________________
Evidence of a chemical reaction: ________________________________________________________________
10. Hydrogen peroxide catalyzed with potassium iodide  ____________ + _____________
_____________
______________ + ________________
Evidence of a chemical reaction: ________________________________________________________________