P.S. Chapter 6 Mini-Labs
Name:_____________
Purpose: To test & demonstrate the Laws & Principles of Chapter 6 in a Lab Setting.
Procedure:
1. The Temperature Lab
a. Mini-Lab Procedure Part 1:
i. Obtain a plastic cup and fill it half full with tap water.
ii. Get a metal backed thermometer and put it in the water to take the temperature.
 Record your temperature in Data Table 1 found below:
iii. Get a small plastic measuring cup and fill it with 5.0 g of Sodium Bicarbonate.
 Use the scale on the West wall and a measuring scoop to measure out 5.0
grams.
iv. Add the Sodium Bicarbonate to your cup of water.
v. Use your thermometer as a stir stick to mix the powder with the water.
vi. Watch the temperature change (it goes up or down {I can’t remember which
though}). When the water temperature has moved as much as it can record the
temperature in Data Table 1.
vii. Get a small plastic measuring cup and fill it with 5.0 g of Calcium Chloride.
 Use the scale on the West wall and a measuring scoop to measure out 5.0
grams.
viii. Add the Calcium Chloride to your cup with the water & Sodium Bicarbonate
mixture.
ix. Use your thermometer as a stir stick to mix the powder with the water.
x. Watch the temperature change (it goes up or down {I can’t remember which
though}). When the water temperature has moved as much as it can record the
temperature in Data Table 1.
xi. Dump out your water – rinse the cup – re-fill the cup with tap water & do Part 2
found below.
b. Mini-Lab Procedure Part 2:
i. Obtain a plastic cup and fill it half full with tap water.
ii. Get a metal backed thermometer and put it in the water to take the temperature.
 Record your temperature in Data Table 1 found below:
iii. Get a small plastic measuring cup and fill it with 5.0 g of Calcium Chloride.
 Use the scale on the West wall and a measuring scoop to measure out 5.0
grams.
iv. Add the Calcium Chloride to your cup of water.
v. Use your thermometer as a stir stick to mix the powder with the water.
vi. Watch the temperature change (it goes up or down {I can’t remember which
though}). When the water temperature has moved as much as it can record the
temperature in Data Table 1.
vii. Get a small plastic measuring cup and fill it with 5.0 g of Sodium Bicarbonate.
 Use the scale on the West wall and a measuring scoop to measure out 5.0
grams.
viii. Add the Sodium Bicarbonate to your cup with the water & Calcium Chloride
mixture.
ix. Use your thermometer as a stir stick to mix the powder with the water.
x. Watch the temperature change (it goes up or down {I can’t remember which
though}). When the water temperature has moved as much as it can record the
temperature in Data Table 1.
What’s in the cup?
Part 1a – Just Water
Temperature (oC)
Part 1a – Water & Sodium Bicarbonate
Part 1a – Water/Sodium Bicarbonate Mixture & Calcium Chloride
Part 1b – Just Water
Part 1b – Water & Calcium Chloride
Part 1b – Water/Calcium Chloride Mixture & Sodium Bicarbonate
c. The Temperature Lab Questions:
i. What signs tell you there is a chemical reaction taking place in Part’s 1a & 1b?
ii. When temperature goes up it’s because the reaction is giving off heat – is this an
Endothermic or Exothermic Reaction?
iii. When temperature goes down it’s because the reaction is absorbing heat – is
this an Endothermic or Exothermic Reaction?
2. The Matter Amounts Lab
a. Make a Prediction: After a Chemical Reaction takes place does the mass of the
reactants increase, decrease or stay the same?
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b. Mini-Lab Procedure:
i. Obtain: two small, plastic, measuring cups & one plastic sandwich bag & Sodium
Bicarbonate & Vinegar (ask Cory for help).
ii. Fill one measuring cup with 5.0 mL of vinegar.
iii. Fill one measuring cup with 5.0 g of Sodium Bicarbonate.
iv. Obtain the total mass of the cups & vinegar & plastic bag.
 Record the total mass here: _________________
v. Place the cups and reactants in the sandwich bag but don’t dump them out and
allow them to react together until the sandwich bag is sealed.
vi. Seal the bag and then shake them up so that they react completely.
vii. What are some signs that there is a chemical reaction?
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viii. Keep the bag sealed and place it on the scale after the reaction has settled down
and find the mass of the reactants.
 Record the total mass here: ______________________
c. Matter Amounts Questions.
i. Compare your mass numbers. Are they the same or different?
ii. How does this compare to your hypothesis?
iii. How does this compare to what Cory tells you should be happening?
3. The Products & Reactants Lab
a. Ask Cory to get you a reaction plate and some chemicals.
i. Chemicals needed: NaCl & KBr & KI & AgNO3.
b. Place three drops of the NaCl into one of the wells of the reaction plate.
c. Onto the NaCl place three drops of AgNO3.
d. Record anything you see or hear into Data Table 2.
e. Place three drops of the KBr into one of the wells of the reaction plate.
f. Onto the KBr place three drops of AgNO3.
g. Record anything you see or hear into Data Table 2.
h. Place three drops of the KI into one of the wells of the reaction plate.
i. Onto the KI place three drops of AgNO3.
j. Record anything you see or hear into Data Table 2.
Data Table 2
Reactant
Reactant
NaCl
AgNO3
KBr
AgNO3
KI
AgNO3
Observations
Product
k. Fill in the “Products” portion of Data Table 2.
l. Answer the following Products & Reactants Questions:
i. What was the most common sign that a reaction had taken place?
ii. Which reaction produced a solid?
Product
iii. Did any reaction make you think the chemicals did not react? Why?
4. The Combining Elements Lab
a. Ask Cory to bring you some Copper powder & an Evaporating Dish.
b. Listen as Cory explains some things about Copper & Oxygen.
c. Make a Prediction: After a Copper reacts with Oxygen does the mass of the reactants
increase, decrease or stay the same?
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d. Place the Evaporating Dish onto the lab scale and measure the mass.
i. Record the mass in Data Table 3 below.
e. Place 2.5 g of Copper into the dish.
i. Record the mass of the Copper & the mass of the Copper & Evaporating Dish
into Data Table 3 where each mass properly belongs.
f. Place the dish with the Copper onto a heating pad on a ring stand under a Bunsen
Burner and cook that dish until the Copper turns black – the color change is super cool
and happens quick so watch it the whole time so you can see what happens.
g. Turn off the gas and leave the dish & copper gunk sit for 10 full minutes to cool down –
Never place a hot anything on a lab scale or it’ll get messed up!
h. After 10 minutes put the dish on the scale and weigh it to see what the new mass is.
i. Record the mass in Data Table 3.
Data Table 3
Evaporating
Dish
Copper Powder
Dish + Copper
Dish +
Black Copper Gunk
Mass (g)
i.
Answer the following questions:
i. Look at your masses in Data Table 3. Do some math and calculate the mass of
just the Black Copper Gunk.
ii. Is the mass of the Black Copper Gunk more, less, or the same as the Copper
Powder?
iii. Cory’s been telling you that mere mortals can’t create matter. Where did the
extra mass come from?
iv. What evidence for a chemical reaction did you observe during heating?
v. That black gunky stuff in the dish is Copper Oxide. Go on the Inter-Web and find
the formula for Copper Oxide.
vi. Look at your masses in Data Table 3. Do some math and calculate the mass of
Oxygen that has been added to the dish.
vii. The reaction of Copper & Oxygen is a Synthesis Reaction – what evidence in this
lab backs up that assertion?
viii. Why do you have to heat the Copper to get it to react with Oxygen in the air?
ix. Sometimes the copper bottoms of cooking pots turns black after the pots are
used. How is this similar to the results in this lab?
5. The Reaction Rates Lab
a. Ask Cory to show you the Paper Clip & Steele Wool Demo
b. Record your observations below:
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c. Go get three little plastic measuring cups. Clean them and dry them out.
d. Fill each cup with 10.0 mL of liquid.
i. One cup gets 10.0 mL of vinegar & 0.0 mL of tap water.
ii. One cup gets 5.0 mL of vinegar & 5.0 mL of tap water.
iii. One cup gets 2.5 mL of vinegar & 7.5 mL of tap water.
e. Into each cup place a small chunk of Magnesium
f. Observe each reaction and describe the reaction rate in Data Table 4 below:
Data Table 4
Reaction Rate
10.0 V & 0 W
5.0 V & 5.0 W
2.5 V & 7.5 W
Observations:
g. Dump your little cups out – liquids down the drain & solids in the trash please.
h. Dry your cups.
i. Use three little plastic measuring cups and set them up so they are all 5.0 mL of Vinegar
& 5.0 mL of Water.
j. Go get three 100 mL glass beakers and fill them up with 80.0 mL of tap water.
i. One cup gets microwaved for 33.0 seconds.
ii. One cup gets two ice cubes added.
iii. One cup gets nothing.
k. Set your little plastic measuring cups into the 80.0 mL of water in the three glass
beakers.
i. DO NOT dump your little plastic cups into the beaker – set them on top so they
float.
ii. Let them float on their water bath for 2.0 minutes so they are at about the same
temperature as the water.
l. Leave the cups floating on their water baths and then add a chunk of Magnesium to
each of your little plastic measuring cups.
m. Observe each reaction and describe the reaction rate in Data Table 5 below:
Data Table 5
Reaction Rate
The Warm One
The Medium One
The Cold One
Observations:
n. Dump your little cups out – liquids down the drain & solids in the trash please.
o. Answer the following questions:
i. When Cory heated the paper clip & the steel wool the heat forced the Iron in both
substances to react with Oxygen in the air. What factor (not the heat)
determined the rate of each reaction? Why?
ii. When you first dropped Magnesium chunks into the cups what factor determined
the rate of each reaction? Why was one greater?
iii. When you dropped Magnesium chunks into the cups at the end what factor
determined the rate of each reaction?
iv. What temperature (hot, medium, cold) most increase reaction rates? Why?