Download Unit 10: Chemical Reactions

Essential Curriculum
Menezes
Unit 10:
Chemical Reactions
Author:
J. Galinski, S. Menezes
Unit 10 Chemical Reactions
Page 1 of 28
Packet Grade: _______/_______
WS: 10pts each
SWS: 20pts each
Reading: 30pts
Introductory Resources:
Addison-Wesley v.5 - Chapter 8
Addison-Wesley v.4 - Chapter 7
Addison-Wesley v.3 - Chapter 7
Main Idea Summary:
 A chemical reaction can be concisely represented by a chemical equation.
 The substances that undergo a chemical reaction are the reactants. The new substances formed are the products.
 Special symbols are written after formulas in equations to show a substance’s state. The designations for solid,
liquid, or gas, are (s), (l), and (g), respectively. A substance dissolved in water is designated (aq).
 A catalyst is a substance that increases reaction rate without being used up by the reaction. If a catalyst is used, its
formula is written above the arrow.
 In accordance with the law of conservation of mass, a chemical equation must be balanced. In balancing an
equation, coefficients are used so the same number of atoms of each element are on each side of the equation.
 In a synthesis reaction, there is always a single product.
 A decomposition reaction involves the breakdown of a single reactant.
 In a single replacement reaction, the reactants and products are an element and a compound. The activity series of
metals can be used to predict whether single replacement reactions will take place.
 A double replacement reaction involves the exchange of cations between two compounds. This reaction generally
takes place between two ionic compounds in aqueous solution. The solubility rules can be used to predict whether
double replacement reactions will take place, and what product will be insoluble in water.
 A combustion reaction always involves oxygen. The products of the complete combustion of a hydrocarbon are
carbon dioxide and water.
 A complete ionic equation shows all dissolved ionic compounds as their free ions. A net-ionic equation shows only
the ions that take part in the actual reaction, and not the spectator ions, ions that do not participate in the reaction.
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Unit 10 Chemical Reactions
Page 2 of 28
Unit 10– Chemical Equations
NAME: _____________________
Laboratory Activity 10A – Balancing Categories Inquiry Activity
A chemical equation sums up what occurs during a chemical reaction. All chemical reactions, whether simple
or complex, desirable or undesirable, involve changing substances. One or more substances, the reactants,
change into one or more new substances, the products. In writing reactions, you separate the reactants from
the products by writing an arrow (→). The arrow means “yields” or “reacts to produce.”
Reactants → Products
Consider for a moment the number of possible chemical reactions. Since there are millions of known
compounds, it is logical to expect that millions of different chemical reactions can occur in nature or be done
in the laboratory. You learned to name many compounds in Unit 07 by following a system of nomenclature
rather than memorizing common names for thousands of different compounds. Similarly, you can learn to
recognize patterns of chemical behavior that allow you to predict the products in many chemical reactions.
Laboratory Activity Instructions:
1.
2.
3.
4.
5.
6.
7.
8.
Form a group of two students.
Get construction paper, scissors, and glue from your instructor.
Cut out the numbered chemical equations from the next page.
Study each of the equations, looking for similarities and patterns.
Based on any similarities or patterns that you recognize, put the equations into categories.
Write out the rules that you used to create the categories on a sheet of paper or notecard.
Glue the rules that you used to the center of the sheet of construction paper.
Glue the equations onto the construction paper near other equations of the same type.
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Unit 10 Chemical Reactions
Page 3 of 28
Unit 10 – Chemical Equations
NAME: _____________________
Laboratory Activity 10A – Balancing Categories Inquiry Activity Equations
(01)
CH4 + 2O2 → CO2 + 2H2O
(02)
H2SO4 + 2KOH → 2H2O + K2SO4
(03)
C2H4 + O2 → CO2 + H2O
(04)
Zn + 2HCl → ZnCl2 + H2
(05)
2Mg + O2 → 2MgO
(06)
2C4H10 + 13O2 → 8CO2 + 10H2O
(07)
Fe + CuSO4 → FeSO4 + Cu
(08)
CaCO3 → CaO + CO2
(09)
BaO + H2O → Ba(OH)2
(10)
H2SO4 → H2O + SO3
(11)
FeS + HCl → FeCl2 + H2S
(12)
2NaCl → 2Na + Cl2
(13)
AgNO3 + NaCl → AgCl + NaNO3
(14)
Pb(NO3)2 + 2 KI → PbI2 + 2KNO3
(15)
2Na + 2H2O → 2NaOH + H2
(16)
MgO + H2O → Mg(OH)2
(17)
C3H8 + O2 → CO2 + H2O
(18) Cl2 + 2NaBr → 2NaCl + Br2
(19) 2Na + Cl2 → 2NaCl
(20) 2KClO3 → 2KCl + 3O2
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Unit 10 Chemical Reactions
Page 4 of 28
Name: _________________________________________ Period: _______________ Date: _________
SWS Word Equations
Word equations: an equation in which the reactants and the products are written by words
Ex: aluminum reacts with oxygen to produce aluminum oxide
Word equation: writing out the chemical names and putting in the correct symbols
aluminum + oxygen → aluminum oxide
Skeleton equation: putting in the correct formulas for the chemical names
Al(s) + O2(g) → Al2O3(s)
Balanced Equation: using coefficients to balance the equation
_4_ Al(s) + _3_ O2(g) → _2_ Al2O3(s)
For each of the following, write the word equation, skeleton equation, and balanced equation.
REMEMBER THE DIATOMIC MOLECULES AND TO CRISS CROSS CHARGES FOR IONIC COMPOUNDS!
1. hydrogen plus oxygen yield water
Word Equation
Skeleton Equation
Balanced Equation
2. nitrogen plus hydrogen yield ammonia
Word Equation
Skeleton Equation
Balanced Equation
3. aluminum bromide plus chloride yield aluminum chloride and bromine
Word Equation
Skeleton Equation
Balanced Equation
4. hydrochloric acid (HCl) plus sodium hydroxide yield sodium chloride plus water
Word Equation
Skeleton Equation
Balanced Equation
5. iron plus lead (II) sulfate react forming iron (II) sulfate plus lead
Word Equation
Skeleton Equation
Balanced Equation
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Unit 10 Chemical Reactions
Page 5 of 28
6. potassium chlorate when heated produces potassium chloride plus oxygen gas
Word Equation
Skeleton Equation
Balanced Equation
7. sulfuric acid decomposes to form sulfur trioxide gas plus water
Word Equation
Skeleton Equation
Balanced Equation
8. sodium oxide combines with water to make sodium hydroxide
Word Equation
Skeleton Equation
Balanced Equation
9. potassium iodide reacts with bromine forming potassium bromide plus iodide
Word Equation
Skeleton Equation
Balanced Equation
10. sodium phosphate reacts with calcium nitrate to produce sodium nitrate plus calcium phosphate
Word Equation
Skeleton Equation
Balanced Equation
11. zinc and chromium (II) nitrate react to form zinc nitrate and chromium
Word Equation
Skeleton Equation
Balanced Equation
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Unit 10 Chemical Reactions
Page 6 of 28
12. hydrogen and nitrogen monoxide produce water and nitrogen
Word Equation
Skeleton Equation
Balanced Equation
13. calcium hydroxide and phosphoric acid yield calcium phosphate and water
Word Equation
Skeleton Equation
Balanced Equation
14. lithium plus oxygen combine to form lithium oxide
Word Equation
Skeleton Equation
Balanced Equation
15. hydrogen reacts with nitrogen to form ammonia
Word Equation
Skeleton Equation
Balanced Equation
16. ethane (C2H6) reacts with oxygen to form carbon dioxide and water
Word Equation
Skeleton Equation
Balanced Equation
17. carbon tetrahydride reacts with oxygen to produce carbon dioxide and water
Word Equation
Skeleton Equation
Balanced Equation
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Unit 10 Chemical Reactions
Page 7 of 28
18. fluorine reacts with sodium chloride to produce sodium fluoride and chlorine
Word Equation
Skeleton Equation
Balanced Equation
19. tricarbon octahydride combines with oxygen to produce carbon dioxide and water
Word Equation
Skeleton Equation
Balanced Equation
20. magnesium sulfide reacts with lithium phosphide to yield magnesium phosphide and lithium sulfide
Word Equation
Skeleton Equation
Balanced Equation
21. copper (II) chloride plus sodium hydroxide produces copper hydroxide and sodium chloride
Word Equation
Skeleton Equation
Balanced Equation
22. zinc (II) chlorate yields zinc chloride and oxygen
Word Equation
Skeleton Equation
Balanced Equation
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Unit 10– Chemical Equations
Worksheet 10.01 – Balancing Basics
Unit 10 Chemical Reactions
Page 8 of 28
NAME: _____________________
Put numbers in the blanks to balance the following equations. Learn to recognize the distinguishing features of each
reaction type.
SYNTHESIS (also known as COMBINATION):
___S + ___O2 → ___SO2
___S + ___O2 → ___SO3
___P + ___O2 → ___P2O5
DECOMPOSITION:
___KClO3 → ___KCl + ___O2
___H2O2 → ___H2O + ___O2
___NaNO3 → ___NaNO2 + ___O2
SINGLE REPLACEMENT (also known as DISPLACEMENT):
___Na + ___H2O → ___NaOH + ___H2
___Zn + ___NaOH → ___Na2ZnO2 + ___H2
___Zn + ___HCl → ___ZnCl2 + ___H2
DOUBLE REPLACEMENT (also known as METATHESIS):
___Fe(OH)3 + ___H2SO4 → ___Fe2(SO4)3 + ___H2O
___MgCl2 + ___NaOH → ___Mg(OH)2 + ___NaCl
___AgNO3 + ___H2S → ___Ag2S + ___HNO3
COMBUSTION:
___C3H8 + ___O2 → ___CO2 + ___H2O
___C6H14 + ___O2 → ___CO2 + ___H2O
___C9H20 + ___O2 → ___CO2 + ___H2O
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Unit 10 Chemical Reactions
Page 9 of 28
Unit 10 – Chemical Equations
NAME: _____________________
Worksheet 10.02 – Synthesis and Decomposition
Put numbers in the blanks to balance the following equations. Learn to recognize the distinguishing features
of each reaction type.
SYNTHESIS (also known as COMBINATION):
___Mg + ___N2 → ___Mg3N2
___N2 + ___O 2 → ___NO 2
___Cu + ___S → ___Cu 2S
___Na + ___O2 → ___Na2O
___Al + ___N2 → ___AlN
___Hg + ___I 2 → ___HgI2
___Fe + ___O 2 → ___Fe2O3
___NO + ___O2 → ___NO2
___H2 + ___Cl2 → ___HCl
DECOMPOSITION:
___HgO → ___Hg + ___O2
___CaCO3 → ___CaO + ___CO2
___CuSO 4∙5H2O → ___CuSO4 + ___H2O
___NH4NO3 → ___N2O + ___H2O
___BaO2 → ___BaO + ___O2
___NO 2 → ___N2 + ___O 2
___H2O → ___H2 + ___O2
___NH3 → ___N2 + ___H2
___NCl3 → ___N2 + ___Cl2
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Unit 10 Chemical Reactions
Page 10 of 28
Lab 10B: Balancing Equations with Gumdrops
Name:___________________________
Introduction
Balancing equations is an essential part of chemistry. If equations were not balanced the Law of
Conservation of Matter would be broken. In this lab you will use gum drops and toothpicks to help
you balance equations.
Materials
Data sheet
Paper towels
Gum drops
Colored pencils
Toothpicks
Procedure
Define the following:
Balance-______________________________________________________________________________
Coefficient- __________________________________________________________________________
Subscript-___________________________________________________________
1. Obtain a bag of gum drops for each color. Each color represents an element.
2. Look at your equation and identify the reactants and products.
3. Using the tooth picks and gum drops construct each compound.
4. On your data sheet make a sketch showing what each compound looks like in the
equation.
5. Now evaluate if your equation is following the Law of Conservation of Matter by identifying the number of each
type of atom for the reactant and product sides.
6. If your equation is not balanced build more compounds using tooth picks and gum drops until it is balanced.
Remember you CANNOT change the compound only how many of each compound.
7. Sketch a picture to reflect how many of each compound was needed to make a balanced equation.
8. Write the balanced equation using chemical formulas and coefficients.
9. Repeat these steps with remaining equations.
Data
H2 + O 2  H2O
Reactants
Chemical
Formula
Sketch
Products
Balanced Equation
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Unit 10 Chemical Reactions
Page 11 of 28
N2 + H 2  NH3
Reactants
Products
Balanced Equation
Chemical
Formula
Sketch
CO2 + H2O  C6H12O6+ O2
Reactants
Products
Balanced Equation
Chemical
Formula
Sketch
P2 + O2  P2O5
Reactants
Products
Balanced Equation
Chemical Formula
Sketch
N2 + Cl2  NCl3
Reactants
Chemical
Formula
Sketch
Products
Balanced Equation
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Unit 10 Chemical Reactions
Page 12 of 28
NAME: _____________________
Worksheet 10.03 – Synthesis Prediction
Use the General Cases to predict the products of each reaction. Balance each equation when done.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
1. Solid beryllium is left in a container with liquid bromine.
2. Solid bismuth is burned in air.
3. Cesium is put in a container with chlorine gas.
4. Phosphorus trichloride is placed in a chlorine rich atmosphere.
5. Solid magnesium oxide is placed in water
6. Sulfur trioxide is bubbled through water.
7. Solid gold is added to fluorine gas.
8. Solid calcium oxide is added to water.
9. Nitrogen monoxide gas is bubbled through water.
10. Hydrogen and oxygen gases are mixed.
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Unit 10 Chemical Reactions
Page 13 of 28
Unit 10 – Chemical Equations
Worksheet 10.04 – Decomposition Prediction
NAME: _____________________
Use the General Cases to predict the products of each reaction. Balance each equation when done.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
1. Potassium hydroxide is heated.
2. Lithium chlorate decomposes by heating.
3. Sodium carbonate is heated.
4. Sulfurous acid is boiled.
5. Molten aluminum chloride is electrolyzed.
6. A sample of magnesium carbonate is heated.
7. A sample of ammonium carbonate is heated.
8. Carbonic acid is boiled.
9. Hydrogen peroxide decomposes.
10. Ammonium hydroxide is heated.
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Unit 10 – Chemical Equations
Laboratory Activity 10C – Synthesis
Unit 10 Chemical Reactions
Page 14 of 28
NAME: _____________________
1. Wear Goggles
2. Observe a strip of magnesium ribbon. Write down any and all observed physical properties.
3. Use the sparklighter to ignite the Bunsen burner.
4. Use the crucible tongs to hold the magnesium ribbon in the Bunsen burner flame. Caution: DO NOT look
directly at the chemical reaction, because it may cause damage to your eyes and permanently harm your
vision. Remove the magnesium from the flame.
5. When the magnesium oxide has cooled, observe its properties.
6. Clean up your equipment and return it to your teacher.
7. Write a balanced equation explaining what happened in lab, causing the transformation of magnesium
into magnesium oxide.
Unit 10– Chemical Equations
Laboratory Activity 10D – Decomposition
1. Wear Goggles.
2. Use a wooden splint to add a pinch of iodine crystals to a plastic cup that is ¾ full of water. Stir with a
stirring rod. Make note of your observations.
3. Use a wooden splint to add a pinch of zinc dust to the same plastic cup. Stir with a stirring rod. Make n ote
of your observations.
4. Attach electrical leads to a 9V battery while the solution settles.
5. Dip the wires into the solution and observe what happens. Record your observations.
6. Hold the wires in place for five minutes. Continue to observe and record.
7. When the reaction has occurred, and all necessary observations have been made, discard the wooden
splints into the trash, discard the zinc iodide solution into the waste container, wash out the plastic cup,
and clean up any other equipment and return it to your teacher.
8. Write a balanced equation explaining what happened in lab, regarding the decomposition of zinc iodide.
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Unit 10 Chemical Reactions
Page 15 of 28
Unit 10 – Chemical Equations
Worksheet 10.05 – Single Replacement
NAME: _____________________
Put numbers in the blanks to balance the following equations. Use the Activity Series to answer the question
at the right. (more reactive replaces less reactive in compounds.)
SINGLE REPLACEMENT (also known as DISPLACEMENT):
REACTION:
WILL IT OCCUR? (Yes or No)
___Fe2O3 + ___Al → ___Al 2O 3 + ___Fe
________
___Al + ___CuSO4 → ___Al2(SO4) 3 + ___Cu
________
___Ca + ___LiNO 3 → ___Li + ___Ca(NO 3)2
________
___Al + ___H2SO4 → ___Al2(SO4)3 + ___H2
________
___Zn(NO3)2 + ___Ag → ___AgNO3 + ___Zn
________
___MgCl2 + ___K → ___KCl + ___Mg
________
___MgCl2 + ___Ag → ___AgCl + ___Mg
________
___Cu + ___AgNO3 → ___Ag + ___Cu(NO3)2
________
___Mn + ___Pb(C2H3O 2)4 → ___Pb + ___Mn(C 2H3O2)2
________
___PtO 2 + ___H2 → ___Pt + ___H 2O
________
___Fe + ___CuSO4 → ___Cu + ___FeSO4
________
___Co + ___Ba(NO3)2 → ___Ba + ___Co(NO3) 2
________
___Hg + ___Pt(OH) 2 → ___Pt + ___Hg(OH)2
________
___Al(C2H3O2) 3 + ___Mg → ___Al + ___Mg(C 2H3O2)2
________
___Sr(NO 3)2 + ___Na → ___NaNO 3 + ___Sr
________
___AlF3 + ___Cl2 → ___AlCl3 + ___F 2
________
___HI + ___Br 2 → ___HBr + ___I 2
________
___Br2 + ___NaCl → ___NaBr + ___Cl 2
________
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Unit 10 Chemical Reactions
Page 16 of 28
Unit 10 – Chemical Equations
Worksheet 10.06 – Single Replacement Prediction
NAME: _____________________
Use the General Cases to predict the products of each reaction. Balance each equation when done.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
1. A piece of copper is dropped into a container of water.
2. Liquid bromine is added to a container of sodium iodide crystals.
3. An aluminum strip is immersed in a solution of silver nitrate.
4. Zinc pellets are added to a sulfuric acid solution.
5. Fluorine gas is bubbled into a solution of aluminum chloride.
6. Magnesium turnings are added to a solution of lead (II) acetate.
7. Iodine crystals are added to a solution of sodium chloride.
8. Calcium metal is added to a solution of nitrous acid.
9. A pea-size piece of lithium is added to water.
10. A solution of iron (III) chloride is poured over a piece of platinum wire.
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Unit 10 – Chemical Equations
SWS Double Replacement
Unit 10 Chemical Reactions
Page 17 of 28
NAME: _____________________
Put numbers in the blanks to balance the following equations. Using the Solubility Rules, predict whether or
not an insoluble product will be formed, and identify the predicted solid precipitate (or if none, the words “no
reaction”) in the blank at the right.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
___Pb(NO3)2 + ___NaBr → ___NaNO3 + ___PbBr2
________
___AgHCO3 + ___NaCl → ___NaHCO 3 + ___AgCl
________
___K2SO4 + ___BaCl2 → ___BaSO4 + ___KCl
________
___Ba(NO3)2 + ___Li2SiF6 → ___BaSiF6 + ___LiNO3
________
___AgF + ___Ca(NO3) 2 → ___AgNO 3 + ___CaF 2
________
___(NH4)2CrO4 + ___Fe(NO3)3 → ___NH4NO3 + ___Fe2(CrO4)3
________
___AgMnO4 + ___KCl → ___AgCl + ___KMnO 4
________
___KOH + ___Al2(SO4)3 → ___Al(OH)3 + ___K2SO4
________
___(NH4)2S + ___SrO → ___(NH 4)2O + ___SrS
________
___AgClO4 + ___NaSCN → ___AgSCN + ___NaClO 4
________
___Na 2CO3 + ___BaCl2 → ___NaCl + ___BaCO 3
________
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Unit 10 – Chemical Equations
WS 10.07 Double Replacement
Unit 10 Chemical Reactions
Page 18 of 28
NAME: _____________________
Put numbers in the blanks to balance the following equations. Using the Solubility Rules, rewrite the
equations as overall equations, ionic equations, and net-ionic equations. Be sure to include identification of
phases, like (s), (l), (g), or (aq) in the reactions.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
___CaCl2 + ___K2CO3 → ___CaCO3 + ___KCl
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___AgNO 3 + ___FeCl3 → ___AgCl + ___Fe(NO3)3
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___Al(OH)3 + ___HC2H3O2 → ___Al(C2H3O2) 3 + ___H2O
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___NaNO3 + ___K2SO3 → No Reaction (Answer the following to demonstrate why)
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
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Unit 10 – Chemical Equations
Worksheet 10.08– Double Replacement II
Unit 10 Chemical Reactions
Page 19 of 28
NAME: _____________________
Put numbers in the blanks to balance the following equations. Using the Solubility Rules, rewrite the
equations as overall equations, ionic equations, and net-ionic equations. Be sure to include identification of
phases, like (s), (l), (g), or (aq) in the reactions.
DOUBLE REPLACEMENT (also known as METATHESIS):
REACTION:
___Na 2SO4 + ___Ba(NO3)2 → ___NaNO 3 + ___BaSO4
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___CuHCO3 + ___KBr → ___CuBr + ___KHCO 3
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___MgCrO4 + ___BaI2 → ___MgI2 + ___BaCrO4
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
___NH4CN + ___Fe(NO3)3 → ___NH4NO3 + ___Fe(CN)3
Ionic Equation:
Spectator Ions:
Net-Ionic Equation:
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Unit 10 Chemical Reactions
Page 20 of 28
Unit 10– Chemical Equations
NAME: _____________________
Worksheet 10.09 – Double Replacement Prediction
Use the General Cases to predict the products of each reaction. Balance each equation when done.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
1. Ammonium sulfate and potassium hydroxide are mixed together.
2. Ammonium sulfide is reacted with hydrochloric acid.
3. Cobalt (II) chloride is combined with silver nitrate.
4. Solid calcium carbonate is reacted with sulfuric acid.
5. Potassium sulfite is reacted with hydrobromic acid.
6. Potassium sulfide is reacted with nitric acid.
7. Ammonium iodide is mixed with magnesium sulfate.
8. Solid titanium (IV) carbonate is added to hydrochloric acid.
9. Solid calcium sulfite is mixed with acetic acid.
10. Strontium hydroxide is added to ammonium sulfide.
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Unit 10 – Chemical Equations
Laboratory Activity 10E – Single Replacement
Unit 10 Chemical Reactions
Page 21 of 28
NAME: _____________________
1. Wear Goggles.
2. Place a test tube in the test tube rack and fill it one third of the way up with 6 M Hydrochloric acid
(WARNING: Hydrochloric acid is very caustic! If you get any on you, wash it off immediately and tell the
teacher).
3. Drop the strip of Magnesium into the acid. Observe what happens. Record your observations.
4. Cover the mouth of the test tube with the second test tube to capture any gas that is produced in the
tube.
5. Use a lit match to test the gas for flammability by putting it in the mouth of the inverted tube.
6. Rinse all glassware thoroughly before returning it.
7. Write a balanced equation for the reaction of magnesium metal with hydrochloric acid. Remember to
include symbols after each chemical formula to represent the phase of each reactant and product. Step 5
of the lab should give a hint as to the identity of one of the products.
Unit 10 – Chemical Equations
Laboratory Activity 10F – Double Replacement
NAME: _____________________
1. Wear Goggles.
2. Observe a solution of Lead (II) Nitrate, Pb(NO3) 2.
3. Fill a test tube about 1/3 of the way up with Pb(NO 3)2.
4. Observe a solution of Barium Chloride, BaCl 2.
5. Add an equal amount of BaCl 2 to the tube.
6. Record your observations of what occurs in the tube for the next several minutes.
7. Write out a balanced equation for what occurs in the tube. Predict the identity of the precipitate.
8. Clean up your station. Discard the contents of the tube in the solution waste container provided by the
teacher.
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Unit 10 – Chemical Equations
SWS Combustion
Unit 10 Chemical Reactions
Page 22 of 28
NAME: _____________________
Put numbers in the blanks to balance the following equations.
COMBUSTION:
REACTION:
___C3H8 + ___O2 → ___CO2 + ___H2O
___C4H10 + ___O2 → ___CO2 + ___H2O
___C5H12 + ___O2 → ___CO2 + ___H2O
___C7H16 + ___O2 → ___CO2 + ___H2O
___C7H14 + ___O2 → ___CO2 + ___H2O
___C9H20 + ___O2 → ___CO2 + ___H2O
___C6H14 + ___O2 → ___CO2 + ___H2O
___CH4 + ___O 2 → ___CO2 + ___H2O
___C2H2 + ___O2 → ___CO2 + ___H2O
___C2H4 + ___O2 → ___CO2 + ___H2O
___C2H6 + ___O2 → ___CO2 + ___H2O
___C8H18 + ___O2 → ___CO2 + ___H2O
___C6H6 + ___O2 → ___CO2 + ___H2O
___C6H12 + ___O2 → ___CO2 + ___H2O
___C6H12O6 + ___O2 → ___CO2 + ___H2O
___C12H22O 11 + ___O2 → ___CO2 + ___H2O
___C8H16 + ___O2 → ___CO2 + ___H2O
___C85H172 + ___O 2 → ___CO2 + ___H2O
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Unit 10 Chemical Reactions
Page 23 of 28
Unit 10 – Chemical Equations
Worksheet 10.10 – Combustion Prediction
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
1. Ethanol is burned completely in air.
2. Propane is heated with oxygen gas.
3. Octane is burned in oxygen gas.
4. Copper (II) Sulfide is burned in air.
5. Solid Phosphorus is burned in air.
6. Barium sulfide is burned in air.
7. Iron is added to an oxygen rich environment.
8. Ethane is burned in oxygen gas.
9. Methane is burned in air.
10. Propanol is burned in air.
NAME: _____________________
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Unit 10 – Chemical Equations
Laboratory Activity 10G – Combustion
Unit 10 Chemical Reactions
Page 24 of 28
NAME: _____________________
1. Wear Goggles.
2. Use a dropper pipet to transfer 10 drops of Ethanol into a watch glass.
3. Drop a lit match into the watch glass and observe the flame.
4. Smother the flame by covering it with an inverted plastic cup. Observe the sides of the cup. What
compound builds up on the sides of the cup?
5. Wash and dry the glassware you used.
6. Ethanol has a formula of CH 3CH2OH. Write a balanced equation for the combustion of ethanol.
Essential Curriculum
Menezes
Unit 10 Chemical Reactions
Page 25 of 28
Unit 10 – Chemical Equations
SWS Basic Predictions
NAME: _____________________
Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify
each reaction type in the blank at the right.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
REACTION:
___C5H12 + ___O2 →
_________________
___Zn + ___HCl →
_________________
___Na 2O →
_________________
___Li + ___Cl2 →
_________________
___Na 2SO4 + ___LiCl →
_________________
___C4H10 + ___O2 →
_________________
___Al2O3 →
_________________
___Al + ___I2 →
_________________
___Zn(OH)2 + ___Al2(CO3) 3 →
_________________
___FeCl3 →
_________________
Essential Curriculum
Menezes
Unit 10 Chemical Reactions
Page 26 of 28
Unit 10– Chemical Equations
Worksheet 10.11 – More Predictions
NAME: _____________________
Use the General Cases to predict the products of each reaction. Balance each equation when done. Identify
each reaction type in the blank at the right.
General Case:
Synthesis:
Decomposition:
Single Replacement:
Double Replacement:
Combustion:
A + B → AB
AB → A + B
AX + B → BX + A
AX + BY → BX + AY
CxHy + O2 → CO2 + H2O
REACTION:
___CuCl2 + ___Na3PO 4 →
_________________
___C12H26 + ___O2 →
_________________
___FeCl3 →
_________________
___K2SO4 + ___Li →
_________________
___Na + ___O2 →
_________________
___C3H8 + ___O2 →
_________________
___KMnO4 + ___Li →
_________________
___Na 3P + ___Ba(OH)2 →
_________________
___H2O →
_________________
___HCl + ___Ca(OH)2 →
_________________
Essential Curriculum
Menezes
Unit 10 – Chemical Equations
SWS– Still More Predictions
Unit 10 Chemical Reactions
Page 27 of 28
NAME: _____________________
Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the
blank at the right.
REACTION:
___Mg + ___O2 →
_________________
___AlCl3 →
_________________
___Na + ___O2 →
_________________
___HCl + ___NaOH →
_________________
___Pb(SO4) 2 + ___Al(C2H3O2)3 →
_________________
___C4H10 + ___O2 →
_________________
___H3PO4 + ___MgCO3 →
_________________
___HgCl2 + ___NaSCN →
_________________
___PtO 2 + ___H2 →
_________________
___CaCO3 + ___NaCl →
_________________
___Ag + ___HNO3 →
_________________
___NCl3 →
_________________
___MgSO 4∙7H2O →
_________________
Essential Curriculum
Menezes
Unit 10 – Chemical Equations
Worksheet 10.12 – Yet More Predictions
Unit 10 Chemical Reactions
Page 28 of 28
NAME: _____________________
Predict the products of each reaction. Balance each equation when done. Identify each reaction type in the
blank at the right.
REACTION:
___Sr + ___O 2 →
________________
___Na + ___H2O →
________________
___Zn + ___HCl →
________________
___ICl →
________________
___Fe(OH)3 + ___H2SO4 →
________________
___C6H14 + ___O2 →
________________
___Au(OH)3 + ___Na2CO3 →
________________
___SrCl2 + ___NaOH →
________________
___OCl2 →
________________
___AgNO 3 + ___H2SO4 →
________________
___Zn + ___O2 →
________________
___Mg(OH)2 + ___NaF →
________________
___C30H62 + ___O2 →
________________
___Mg(NO3)2 + ___H2O →
________________
___Au2S3 →
________________
___Ti(MnO4)4 + ___Fe2O 3 →
________________
___MnF2 + ___O2 →
________________
___CO2 →
________________