Grade 10 Chem. CPT:
Chemical Reactions & Types
Date: ___________
Introduction: This is the culminating task for your chemistry unit. This task will require you to apply your
understanding of chemical nomenclature, identifying chemical reactions, writing chemical formulas and
balancing equations. In this experiment, you will investigate ten different chemical reactions. One lab
report per group.
Learning Goals:
1) Conduct chemical reactions safely
2) Observe the reactions and record the signs of a chemical reaction
3) By observing chemical reactions, we shall:
a)
b)
c)
d)
e)
Safety Considerations:
Lab Report:
Provide qualitative observations before, during, and after the chemical reaction
Determine the type of chemical reaction
Write a word equation
Write a skeleton equation (unbalanced chemical equation with states)
Write balanced chemical equations
Put on goggles and apron upon entering the room and must stay on until all groups have
returned their chemicals to the cart. Tie long hair back. This lab involves corrosive,
toxic and flammable chemicals – so care must be taken throughout this lab. Stay at your
desk until the teacher tells you to move to the next station. More safety considerations
are discussed in the procedure!
You will write a report for each chemical reaction. The following is an example of what you will write in
each report… “Always remember report speech”
EXAMPLE:
Reaction #1: Pour 3 mL of potassium iodide solution and 3 mL of lead (II) nitrate
solution into a test tube. Record your observations.
Prior to mixing, potassium iodide was a clear, light yellow solution and lead (II) nitrate
was a white, translucent (cloudy) solution. When the two solutions were mixed a bright
yellow precipitate formed and the remaining solution was translucent and light yellow
in colour.
Potassium iodide(aq) + Lead (II) nitrate(aq)  Potassium nitrate(aq) + Lead (II) iodide(s)
2 KI(aq) + Pb(NO3)2(aq)  2 KNO3(aq) + PbI2(s)
(double displacement)
Assessment Tips:




The lab reports should be neat, organized, and easy to read
Be sure to use as much scientific terminology as possible in order to receive full communication marks
Read over each lab report to make sure you have completed all sections
Be sure to put your name on each page that you fill out

My assigned group members are (3):
a)
b)
c)
d)
_____________________________________________________
_____________________________________________________
_____________________________________________________
_____________________________________________________
Procedure:
Reaction A:
1.
Attach the hose of the Bunsen burner to the gas nozzle. Open the Bunsen burner to allow high gas flow.
2.
Turn on the gas by turning the valve handle until it is parallel with the gas nozzle. Use the sparker to ignite the
flame.
3.
Adjust the flow of gas until you see a blue flame about 2 or 3 cm high surrounded by a cooler, lighter- coloured
flame. Note the sound of the flame. Describe the chemical reaction taking place.
Reaction B:
1.
Place enough sulfur (S8) to cover the Queen’s head on a shiny copper coin.
2.
Using tongs, gently heat the coin in the Bunsen burner flame until the sulfur melts and burns. Describe any
changes in the appearance of the coin.
Reaction C:
1.
Use tweezers to add a piece of magnesium to a test tube half-filled with 0.5 or 1.0 mol/L hydrochloric acid (HCl).
Cover the mouth of the test tube for 30 seconds, bring the mouth of the test tube to a flame (burning splint).
Record your observations. Extract remaining Mg and pour contents into waste beaker.
Reaction D:
1.
Ignite a 6 cm piece of magnesium ribbon in the candle or burner flame. (CAUTION: Do not look directly at the
burning magnesium!)
2.
Compare the materials before and after burning.
Reaction E:
1.
Describe the iron nitrate (Fe(NO3)3) and potassium hydroxide (KOH) solutions.
2.
Add ¼ test tube of potassium hydroxide solution to ¼ test tube iron nitrate solution.
3.
Describe the reaction. Pour waste materials into waste beaker.
Reaction F:
1.
Place a piece of cleaned copper wire into a test tube ¼ filled with silver nitrate solution. Leave for 5 minutes then
observe. (CAUTION: Do not get silver nitrate on your hands or clothes!).
2.
Describe what happens to the copper in the silver nitrate solution.
Reaction G:
1.
Add ¼ test tube of sodium carbonate solution to ¼ test tube of magnesium chloride solution.
2.
Describe the solutions before and after mixing.
3.
Pour waste materials into waste beaker.
Reaction H:
1.
This is the toughest reaction to determine. Pour about 10 ml of distilled water into a test tube (½ full).
2.
Add 3 or 4 drops of universal indicator to the distilled water.
3.
The water will change colour to indicate pH. See the chart to indicate which colour corresponds to which
particular pH level.
4.
Add enough calcium chloride granules to fill the test tube to a depth of 1 cm. Describe the reaction. Note: if pH
rises a base has been produced, if pH lowers an acid has been produced. DO NOT SHAKE THE TEST TUBE!
Remember to put all waste chemicals into the waste beakers provided at each desk. Do not pour the chemicals down
the sink. Clean the desk of the last station you visited. Return all equipment aprons, protective goggles and unused
chemicals to the front of the class.
Reaction I:
1.
2.
Pour about 5 ml (¼ test tube) of ethanol into an evaporating dish.
Ignite the ethanol with a match or flaming splint. Observe the flames until the ethanol has completely burned.
Reaction J:
1.
2.
3.
4.
5.
Teacher demonstration for the whole class
Teacher demonstration for the whole class
Add 50 mL of 35% V/V hydrogen peroxide (H2O2) to a 1000 mL graduated cylinder.
Place the graduated cylinder into a large, shallow plastic tub.
Add about 5 to 10 ml of liquid dish detergent to the graduated cylinder
Add about 5 to 10 crystals of potassium iodide (KI) to the hydrogen peroxide (H2O2) (Note: The KI is a catalyst
and does not partcicpate in the Chemical Reaction)
Place a glowing wooden splint in the foam while the reaction is occurring. Observe the reaction.
Grade 10 – Types of Chemical Reactions SOLUTIONS
Reaction 1
methane + oxygen  carbon dioxide + water
CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(g)
synthesis – combustion
Reaction 2
copper + silver nitrate  copper(II) nitrate + silver
Cu(s) + 2 AgNO3(aq)  Cu(NO3)2(aq) + 2 Ag(s)
single displacement
Reaction 3
magnesium + hydrochloric acid  magnesium chloride + hydrogen
Mg(s) + 2 HCl(aq)  MgCl2(aq) + H2(g)
single displacement
Reaction 4
iron(III) nitrate + potassium hydroxide  potassium nitrate + iron(III) hydroxide
Fe(NO3)3(aq) + 3 KOH(aq)  3 KNO3(aq) + Fe(OH)3(s)
double displacement
Reaction 5
Copper(II) sulphate + Iron filings  Iron(II) sulphate + Copper
CuSO4(aq) + Fe(s)  FeSO4(aq) + Cu(s)
(Single Displacement)
Reaction 6
hydrogen peroxide  water + oxygen
MnO2(s)
2 H2O2(aq)

2 H2O(l) + O2(g)
decomposition
Reaction 7
ethanol + oxygen  carbon dioxide + water
C2H5OH(aq) + 3 O2(g)  2 CO2(g) + 3 H2O(g)
synthesis – combustion
Reaction 8
sodium carbonate + magnesium chloride  sodium chloride + magnesium carbonate
Na2CO3(aq) + MgCl2(aq)  2 NaCl(aq) + MgCO3(s)
double displacement
Reaction 9
Calcium chloride + water  hydrochloric acid + calcium hydroxide
CaCl2(s) + H2O(l)  HCl(aq) + Ca(OH)2(s)
Double displacement