unit 5 percent composition, empirical formulas & reactions · using the element with the...
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Unit 5Percent Composition, Empirical Formulas & Reactions
CHAPTERS 10 & 11
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Percent Composition of a Compound
SECTION 10.3
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Math Warm Up
What is 73% of 150?
109.5
What percentage of 6.5 is 3.1?
48%
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Percent Composition1. Calculating % from experimental data
Based on mass (not moles or # of particles)
For a compound it depends on the formula:
When a 13.60 g sample of a compound containing only magnesium and oxygen is decomposed, 5.40 g of oxygen is obtained. What is the percent composition of this compound?
%100% xMass
MassMass
Compound
Element
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2. Calculating % from formulas and molar mass
% mass = molar mass of element X 100%
molar mass of compound
What is the percent composition of the elements in Propane (C3H8)?
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3. Percent composition as a conversion factor
How many grams of Carbon and Hydrogen are in 82.0 g of C3H8?
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Hydrated Crystals
CoCl2●6H2O Hydrated Crystal
CoCl2 Anhydrous Crystal
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Example Problem
What is the percent of water in Cobalt (II) chloride hexahydrate?
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Warm-up 1/19
Hydrogen peroxide has the formula H2O2. What percent is it H, and what percent is it O?
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Empirical Formulas
Formula Units ARE Empirical Formulas
Examples
NaCl
(NH4)2SO4
Molecular Formulas are not necessarily Empirical Formulas
Examples
C2H6
H2O2
H2O
• Lowest whole number ratio of elements in a compound
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Identify each compound as Molecular or Ionic. Which ones are also “Empirical Formulas”?
Mg3(PO4)2
C6H12O6
CO
CaCl2
C6H6
H2O
(NH4)2CO3
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Calculating Empirical Formulas
1. Find mass of each element in a compound
2. Convert masses to moles
3. Using the element with the smallest number of moles – Calculate the whole number “mole ratio” of each element (Divide each mole value by the smallest)
Example: 52.9% Aluminum 47.1% Oxygen
52.9 g Aluminum 47.1 g Oxygen52.9 g Al (1mol/26.98 g) = 1.96 mol Al 47.1 g O (1 mol/16.0g) = 2.94 mol O
52.9 g Aluminum 47.1 g Oxygen52.9 g Al (1mol/26.98 g) = 1.96 mol Al 47.1 g O (1 mol/16.0g) = 2.94 mol O
1.96 mol Al / 1.96 = 1 mol Al 2.94 mol O/ 1.96 mol = 1.5 mol O
Empirical Formula: Need to multiply each by 2 to turn into whole numbers Al2O3
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Example
What is the empirical formula for a compound which contains 41.1% iron, 23.6% sulfur and 35.3% oxygen?
First assume each % is a mass in g’s (corresponding to a total substance mass of 100.00 g). Find the atomic mass of each element from the periodic table and use it to convert the mass in grams to moles.
41.1 g Fe Fe: 55.85 g/mol (41.1g)/(55.85g/mol) = 0.736 mol Fe
23.6 g S S: 32.07 g/mol (23.6g)/(32.07g/mol) = 0.736 mol S
35.3 g O O: 16.00 g/mol (35.3g)/(16.00g/mol) = 2.21 mol O
Next, convert the mole values to lowest whole number mole ratios. Do this by dividing each mole value by the smallest mole value of the group. These whole numbers tell the empirical formula ratios.
0.736 mol Fe 0.736mol/0.736mol = 1
0.736 mol S 0.736mol/0.736mol = 1
2.21 mol O 2.21 mol/0.736 mol = 3
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Warm-up 9/20
What is the empirical formula of a compound that is 40.7% Carbon, 5.1% Hydrogen, and 54.2% Oxygen?
What is the molar mass of this formula?
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Calculating Molecular formula
Divide the molar mass of the molecular formula by the molar mass of the empirical formula. The answer represents the factor the empirical formula needs to multiplied by.
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Molecular Formulas
Look at Problem # 15a on Worksheet 1
15. Determine the molecular formula for a compound: (Hint: you will need to calculate the empirical formula first)
a. 94.1% O and 5.9% H: Molar mass = 34 g/mol
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Ch 11Describing Chemical Reactions
Introduction to Chemical Equations
ALL chemical reactions follow 2 laws!
Law of Conservation of mass:
In a chemical reaction, the total mass of the reactants and the total mass of the products must be the same.
Law of Conservation of Atoms:
In a chemical reaction, atoms can not be created or destroyed.
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Chemical Reactions are about the arrangement of Atoms, Not the changing of Atoms
The only thing about atoms that changes to drive chemistry is the location of electrons
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Reaction Vocabulary:
Reactants: Starting Atoms, Molecules, or Compounds
Products: Ending Atoms, Molecules, or Compounds
Yields: Progress of reaction – Gives “→”
Catalyst: Substance that speeds up chemical reactions
Additional Information
States of Matter
Shown as (s), (l), (g), (aq) after formulas
Catalyst
Shown above Yield arrow
If Heat is added show with or H above Yield arrow
CatalystReactants Products
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Example:
Aqueous hydrogen peroxide will decompose into gaseous forms of oxygen and water in the presence of manganese dioxide as a catalyst
)(2)(2)(222
gg
MnO
aqOHOOH
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Balancing Chemical EquationsFollowing the Law of conservation of ATOMS You must NEVER change the # of Atoms in a formula by changing the
subscript numbers
To change # of atoms (or molecules or compounds), add a coefficient
Coefficients are numbers placed in front of a formula.
Coefficients change the # of atoms by a multiplying effect
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Example:
Hydrogen gas combusts with Oxygen gas to form water.
1. Get Formulas correct
2. Organize REACTANTS vs. PRODUCTS
3. BALANCE
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Balancing Reaction HINTS
Look for Polyatomic Ions!
Save elements O2 and H2 for the end.
If you assume the coefficient of a large particle is 1 and come to a dead end, change it to a 2.
Mg3(PO4)2 + NaCl MgCl2 + Na3PO4
C2H6 + O2 CO2 + H2O
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Reaction Types
1. Combination Reaction:
2 or more substances as Reactants combine to form 1 Product
Also Called “Synthesis”
2. Decomposition Reaction:
1 Reactant breaks down into 2 or more Reactants
Most require energy to take place (take in Energy)
3. Single-Replacement Reaction:
1 element replaces another element in a compound
Reactivity of Metals and Non-Metals is important:
Use activity series (Page 361).
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4. Double-Replacement Reaction:
An Exchange of positive ions between 2 Ionic Compounds
Both Reactants are Ionic Compounds
Often takes place in solution with water.
Sometimes a Product is a solid that will not dissolve in water and forms a PRECIPITATE
5. Combustion Reactions
A Reactant combines with Oxygen (other Reactant)
Usually produce energy (give off energy)
Usually involves a Molecular Compounds with (C,H, & or O) and Oxygen
Often have Water and Carbon dioxide as Products
“Burning Hydrocarbons”
Wood, Gas, Fuel, Sugars (Remember Cellular Respiration?)
May also be a Combination (synthesis) Reaction if only one Product forms
“Burning Elements”
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Combination:
A + B AB
Decomposition:
AB A + B
Single Replacement:
AB + C CB + A
Double Replacement:
AB + CD AD + CB
Combustion:
? + O2 H2O + CO2
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Predicting Reaction Types Examples
1. A single Reactant: H2O2
2. A metal (Na) and an Ionic Compound (MgCl2) React:
3. C2H6 reacts with O2:
4. Two Ionic compounds react [KCl & Mg(NO3)2]
5. A single product: H2O