chemical reactions and equations. chemical change - objectives 1. list the common indicators of a...
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Chemical ReactionsAnd Equations
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Chemical Change - objectives
1. List the common indicators of a chemical change and use them to identify when a chemical reaction has probably occurred. They are: color change, change of state (gas bubbles, precipitate, etc), temperature change, pressure change in a closed container, and change in odor. Note the emphasis on change
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Indications of a Chemical ReactionThere are some easily observed changes that usually indicate a chemical reaction1.Color change2.Change of state (gas bubbles, precipitate, etc), 3.Temperature change4.Pressure change in a closed container5.Change in odor
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1. Color change
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2. Change of state: gas bubbles
Release of gas bubbles when two substances mixed is often evidence of chemical reaction
Antacid in water
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2. Change of state: formation of precipitate
Many reactions happen in solution
If solid appears after two solutions mixed, a reaction has probably happened
Example: Pb(NO3)2 + KI
A bright yellow solid PbI2 appears as the proof that the reaction has happened
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2. Change of state: formation of precipitate The solid that appears
is called precipitate Precipitate a solid
that is made as a result of a chemical reaction in solution and that separates from the solution
PbI2 precipitate
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3. Temperature change
Note: Heat by itself NOT necessarily sign of chemical change
Reaction between vinegar and baking soda is accompanied by drop of temperature
Reaction between glycerin C3H5(OH)3 and potassium permanganate KMnO4 produces extensive heat (burning)
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4. Pressure change in a closed containerIf reaction is going in the gas phase and new gases are formed, the pressure in the closed container will change
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5. Odor change
Odor Changes It only takes one experience with a rotten egg to learn that they smell different that fresh eggs. When eggs and food spoil, they undergo a chemical change. The change in odor is a clue to the chemical change
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Understanding Check
Is it a chemical or physical change?1. “Dry ice”, solid carbon dioxide, is sublimated into
gaseous CO2 at room temperature
2. Salt is dissolved in water3. Iron rusts in a damp environment4. Gasoline burns in the presence of oxygen5. Liquid hydrogen peroxide (H2O2) decomposes to water
and oxygen6. Rotting of eggs
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Chemical Equations - objective2. Given a word equation, write a chemical equation (this requires good formula writing skills)
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Chemical reaction is a process by which one or more substances are changed into one or more different substances
Chemical equations represent chemical reaction with symbols and formulas. Chemical equations show the identities, physical phases and relative amounts of the reactants and products in a chemical reaction
Reactants (state) → Products (state) Reactants are compounds being brought together to react Products are the new compounds that are made in the reaction
Chemical Reactions and Equations
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Physical Phase
•Solid (s)•Liquid (l)•Gas (g)•Aqueous solution (aq) – solution in water
•Examples: Na (s); O2 (g); HCl (l); Ca(NO3)2 (aq)
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Word Equations First step in writing chemical equation is to identify
facts to be represented Word equation “equation” in which reactants and
products are represented by words Does not give quantities of reactants/products
Reactants ==> Productschemicals that react ==> chemicals that are produced
hydrogen + oxygen ==> waterhydrogen peroxide ==> water + oxygenmagnesium + oxygen ==> magnesium oxidesodium chloride ==> sodium + chlorine
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Formula Equations
Word equation: hydrogen (gas) + oxygen (gas) water (liquid)Formula equation: H2 (g) + O2 (g) H2O (l)
magnesium (solid) + oxygen (gas) magnesium oxide (solid)
Mg (s) + O2 (g) MgO (s)
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Characteristics of Chemical Equations1. The equation must contain correct formulas for the
reactants and products.2. The Law of Conservation of Mass must be satisfied:
mass is neither created nor destroyed in any ordinary chemical reaction. • The quantity of substances produced (products)
by a chemical reaction is always equal to the quantity of the reacting substances (reactants).
• The “quantity” here means mass or the number of atoms for each element participating in reaction
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Balancing a Chemical Equation1. Write a formula equation
H2O(l) H2(g) + O2(g)
2. Create a table showing the number of atoms for each element: This equation is not balanced!The number
of atomsReactants Products
H 2 2
O 1 2
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Balancing Equations3. Correct the number of O by placing coefficient 2 in front of H2O2H2O(l) H2(g) + O2(g)
4. Correct the table:
Oxygen is now balance with 2 on left and 2 on right. H is not!5. Now balance hydrogen – 4 on left, 2 on right. Add coefficient 2 to H2
2H2O(l) 2H2(g) + O2(g) balanced!
The number of atoms
Reactants Products
H 4 2
O 2 2
The number of atoms
Reactants Products
H 4 4
O 2 2
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Guidelines for Balancing Equations Create a table of elements for reactant and product
side of the equation Balance the different types of atoms one at a time. First balance the atoms of elements that are
combined and that appear only once on each side of the equation.
Balance polyatomic ions that appear on both sides as single units.
Balance lone atoms, especially H and O atoms (or any), last.
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DO NOT!!!.....
• DO NOT WRITE INCORRECT FORMULAS, THIS WILL MESS UP YOUR BALANCING
• DO NOT CHANGE SUBSCRIPTS IN FORMULAS TO BALANCE THE EQUATION!
H2O(l) H2(g) + O2(g) H2O(l) H2(g) + O(g)
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DO!.....
• When you think you have balanced the equation, COUNT THE NUMBERS OF EACH TYPE OF ATOM ON EITHER SIDE OF THE EQUATION
2H2O(l) 2H2(g) + O2(g)
Reactant side Product sideH 4 4O 2 2
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Sample Problem 1Write balanced chemical equations for the following reaction: Solid sodium combines with chlorine gas to produce solid sodium chloride.•Word reaction:Sodium (solid) + chlorine (gas) sodium chloride (s)•Formula reaction:Na(s) + Cl2(g) → NaCl(s)
•Balanced reaction2Na(s) + Cl2(g) → 2NaCl(s)
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Balance ReactionNa(s) + Cl2(g) → NaCl(s)
1.Count atoms:1. Na (in compound): 1 on the left, 1 on the right - balanced2. Cl (lone element): 2 on the left, 1 on the right – not balanced!
2.Adjust Cl: Na(s) + Cl2(g) → 2 NaCl(s)
Count atoms:1. Na: 1 on the left, 2 on the right – not balanced!2. Cl: 2 on the left, 2 on the right – balanced
3.Adjust Na: 2 Na(s) + Cl2(g) → 2 NaCl(s)
Count atoms – all balanced!1. Na: 2 on the left, 2 on the right2. Cl: 2 on the left, 2 on the right
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Sample Problem 2Write word, formula, and balanced chemical equations for magnesium and hydrochloric acid (HCl) react to produce magnesium chloride and hydrogen.Word equation: Magnesium (solid) + hydrochloric acid (liquid) magnesium chloride (solid) + hydrogen (gas)Formula equation: Mg (s) + HCl (l) MgCl2 (s) + H2 (g)Count atoms:
1. Mg (in compound): 1 on the left, 1 on the right2. Cl (in compound): 1 on the left, 2 on the right3. H (lone element): 1 on the left, 2 on the right
Adjust HCl: Mg + 2HCl MgCl2 + H2
Recount the atoms – all balanced!
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Word equation: Methane (gas) + oxygen (gas) carbon dioxide (gas) + water (gas)
Formula equation: CH4(g) + O2(g) CO2(g) + H2O(g)
Sample Problem 3
Reactants Products Balanced?
1. C (in compounds in both sides) 1 1 Yes
2. H (in compound) 4 2 No
3. O (in compound and a lone element)
2 3 No
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• Adjust H: CH4(g) + O2(g) CO2(g) + 2H2O(g)
• Adjust O: CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
Sample Problem 3 (cont.)
Reactants Products Balanced?
1. C (in compounds in both sides) 1 1 Yes
2. H (in compound) 4 4 Yes
3. O (in compound and a lone element)
4 4 Yes
Reactants Products Balanced?
1. C (in compounds in both sides) 1 1 Yes
2. H (in compound) 4 4 Yes
3. O (in compound and a lone element)
2 4 No
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Practice Problems
Fe + Cl2 = FeCl3
2Fe + 3Cl2 = 2FeCl3
Zn + HCl ZnCl2 + H2
Zn + 2HCl ZnCl2 + H2
Al + O2 Al2O3
4Al + 3O2 2Al2O3