Types of Chemical Reactions:
Chemistry is the study of matter and how it reacts. In this lab, you will observe
reactions between substances and explore the relationship between your
observations and the chemical shorthand used to represent these reactions.
Objective: I will observe a series of chemical reactions and will classify them into
various categories of reactions I learned.
Safety Consideration
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Follow all laboratory safety procedures.
Wear goggles at all times.
Dispose of chemicals in the manner indicated by your teacher.
Do not to contaminate the solutions.
Materials used:
Make a list of all the apparatus used and chemicals used in this experiment.
Data Collection
For each reaction, record the following data observations:
1. List the name and formula of each reactant.
2. Note the physical characteristics of each reactant, including color (but not
red as red is not a true color), phase, etc.
3. Describe any evidence for chemical change you observe.
4. Note the physical characteristics of each product, including, phase, etc.
5. Write a complete balanced chemical equation for the process, including
substance phases (solid, liquid, gas, aqueous, (and plasma)), and input
energy or presence of a catalyst.
6. Note the type of the chemical reaction under which the process falls.
Identify the gases
You will observe evolution of three gases during this lab, Oxygen, hydrogen and
carbon dioxide.
1. The test for oxygen is, it helps in combustion so a glowing splint will light up
when brought in contact with the gas.
2. Hydrogen: is explosive so a burning splint will pop in the presence of
Hydrogen
3. Carbon dioxide is a fire extinguisher. If you bring a burning splint close to
the gas it will go off.
Questions:
1. During which experiment a catalyst was used? What was the role of the
catalyst?
2. During which experiment/s Carbon dioxide gas was released? How did
you test for this gas?
3. During which experiment/s Hydrogen gas was released? How did you test
for this gas?
4. During which experiment/s Oxygen gas was released? How did you test
for this gas?
5. During which experiment a heat was lost or gained? Classify as
exothermic or endothermic?
6. Which experiment you liked the most?
Conclusion:
Write a full page written or half page typed conclusion at the end of the
experiment stating if you met your objectives? Your opinion, what did you learn,
how you can modify it, what was good and bad about this experiment.
Reaction 01:
1. Hold a piece of magnesium (provided by your teacher)
with a pair of tongs.
2. Light the Bunsen burner using a striker. Now light the
magnesium using Bunsen burner flame, and drop the
piece of magnesium into an aluminum can. NOTE: Do
not look directly into the burning flame as it could
damage your eyes (or cause you to have a reaction like
the Nazis in Raiders of the Lost Ark, it’s 50/50)
3. Examine the residue, which is the product of this
reaction.
Reaction 02:
1. Fill a test tube with around ¼ t-spoon sulfur powder
(Don’t sniff the sulfur powder either).
2. Heat the filled test tube over a Bunsen burner flame.
Use the test tube clamp to hold the test tube.
3. Use tongs to drop the copper strip (provided by your
teacher) into the sulfur. Look for evidence of a change
when the copper is added to the sulfur.
4. Examine the cooled copper foil for presence of the
product of this synthesis reaction.
Reaction 03:
1. Fill a test tube, approximately halfway, with distilled
water.
2. Add 2 drops of Bromothymol Blue or Universal
Indicator. Either substance works fine.
3. Insert a straw into the test tube and blow into the water
(Do not drink the water)
4. Observe evidence for the reaction of the water and
carbon dioxide
Reaction 04:
1. Fill a test tube, approximately halfway, with distilled
water.
2. Add 2 drops of phenolphthalein Indicator.
3. Add about 0.01 g (don’t weigh just estimate) of
Calcium oxide to the test tube.
4. Observe the test tube for evidence of the reaction
between Calcium oxide and water.
Reaction 05:
1. Fill a test tube, approximately halfway, with
Hydrogen Peroxide.
2. Observe the test tube for evidence that the
hydrogen peroxide is decomposing.
3. Add 0.05 g (don’t weigh just estimate) of
Manganese (IV) oxide to the test tube which acts as
a catalyst for the decomposition reaction.
4. Observe the test tube for evidence for the
decomposition of hydrogen Peroxide.
Reaction 6:
1. Add 3 ml (a dropper full) of Silver nitrate solution to a test
tube.
2. Use tongs to drop the copper wire strip (provided by your
teacher)in the silver Nitrate solution.
3. Observe the contents of the test tube for evidence of a
reaction between the two substances.
Reaction 7:
1. Add 3 ml of Copper Chloride(a dropper full) solution to a
test tube.
2. Cut a narrow strip of Aluminum Foil, about 8
centimeters long.
3. Use tongs to drop the Aluminum foil into copper
Chloride solution.
4. Observe the contents of the test tube for evidence of a
reaction between the two substances.
Reaction 8:
1. Add 5 ml of Acetic acid (Vinegar) solution to a test
tube.
2. Weigh 5 g of Sodium bicarbonate (baking soda) and
add to the test tube.
3. Observe the contents of the test tube for evidence of
a reaction between the two substances.
Reaction 9:
1. Add 5 ml of Sodium Chloride solution to a test
tube.
2. Add 2 ml (half dropper full) of Silver Nitrate to the
test tube.
3. Observe the contents of the test tube for evidence
of a reaction between the two substances.
Reaction 10:
1. Add 3 ml (a dropper full) of Lead Nitrate solution to a test
tube.
2. Add 3 ml (a dropper full) of Potassium iodide solution to
the same test tube.
3. Observe the contents of the test tube for evidence of a
reaction between the two substances.
Reaction 11:
1. Add 5 ml (a dropper full) of Copper Sulfate solution to a
test tube.
2. Add 5 ml of NaOH(a dropper full) solution to the same
test tube.
3. Observe the contents of the test tube for evidence of a
reaction between the two substances.
Reaction 12:
1. Add 5 ml of Copper Sulfate solution to a test tube.
2. Add about 2 grams (estimate don’t weigh) of Iron
Fillings into the same test tube.
3. Wait for 2 minutes for the reaction to occur.
4. Observe the contents of the test tube for evidence of a
reaction between the two substances.
Reaction 13:
1. Add 5 ml of Hydrochloric acid to a test tube.
2. Take two pieces of Zinc metal and drop them in the same
test tube. (Use tongs to drop the Zinc metal into
Hydrochloric acid solution).
3. Observe the contents of the test tube for evidence of a
reaction between the two substances.
4. Identify the gas coming out using a burning wooden splint
and observe what happens?
Reaction 14:
1. Add 5 ml of Hydrochloric acid to a test tube.
2. Take two pieces of Magnesium ribbon (ask your teacher
for Mg ribbon) and drop them in the same test tube.
(Use tongs to drop the Mg ribbon into Hydrochloric acid
solution).
3. Observe the contents of the test tube for evidence of a
reaction between the two substances.
4. Identify the gas coming out using a burning wooden
splint and observe what happens?
Reaction 15:
1. Fill a test tube, approximately halfway, with Sodium
bicarbonate (baking soda).
2. Heat the test tube in the flame holding the test tube
with test tube tongs.
3. Observe the test tube for evidence that Sodium
bicarbonate (baking soda) is decomposing.
4. Observe the test tube for evidence for the gas coming
out.
5. Identify the test via testing it using a burning splint.
Reaction 16:
1. Fill a test tube, approximately halfway, with Sugar.
2. Heat the test tube in the flame holding the test tube
with test tube tongs.
3. Observe the test tube for evidence that Sugar
decomposing.
4. Observe the test tube for evidence for the gas coming
out.
5. Identify the test via testing it using a burning splint.