Post on 14-Jan-2016
2.C – Conserving Matter
Do Now
How many and what type of atoms are in the following examples:CH4
4NH3
6Ca(OH)2
Objectives
1. SWBAT define the law of conservation of mass.
2. SWBAT review reactants, products, coeiffients, and determining the number of atoms in a given formula.
3. SWBAT balance chemical equations with a partner.
When a car’s gas empties, where do the atoms in the gasoline go?
Keeping Track of Atoms
Law of Conservation of Matter: Matter is neither created nor destroyed.
Since chemical reactions cannot create or destroy atoms, chemical equations representing the reactions must always be BALANCED.
Atomic Perspective:
C O2 CO2
1 Carbon atom 1 oxygen molecule 1 carbon dioxide molecule
1. What are the reactants in this chemical equation?
2. What are the products in this chemical equation?
3. Are there the same number of atoms on both sides of the equation?
a. Where any atoms destroyed or created?
b. Was the Law of Conservation of Matter maintained?
2 Cu (s) + O2 (g) 2 CuO (s)
COEFFICIENTS - indicates the number of units of each substance involved.
1. Does the oxygen molecule have a coefficient?
2. What do the subscripts represent?
3. Can subscripts be removed from chemical equations?
How do we Balance Equations?
2 H2 + O2 2 H2O
Subscripts
Coefficients
# of atoms in a compound
Number of compounds in the reaction
Subscripts balance charges within a compound.
Coefficients balance atoms in an equation
What do Coefficients Really Mean?
CH4 + 2 O2 CO2 + 2 H2O
Total:1 C4 H4 O
Total:1 C4 H4 O
The equation is balanced.
H
C
H
HH
O O
O O
CO O HO
H
HO
H
H
CC
H
HH
O O
O O
CCO O HO
H
HO
H
Make an atom inventory for the following equation
Al2O3 + HCl -> AlCl3 + H2O
Is it Balanced?
SWBAT
Practice balancing equations in groups.
Taken from Kelly Deters
Make a table of elements
_____ __________
How to Balance By Inspection:
1
Reactants Products
H
O
C
CH4 + O2 H2 O CO2+_____
Taken from Kelly Deters
2 Count the number of each element or ion on the reactants and products side.
_____ __________
How to Balance By Inspection:
Reactants Products
H
O
4
2 3
2
C 1 1
CH4 + O2 H2 O CO2+_____
Don’t forget to add all the atoms of the same element together—even if it appears in more than one compound!
Taken from Kelly Deters
3Each time you add a coefficient, update your table with the new quantities of each atom.
Add coefficients to balance the numbers
_____ __________2
How to Balance By Inspection:
Reactants Products
H
O
4
2 3
2
C 1 1
2
4
44
CH4 + O2 _____ H2 O CO2+
Taken from Kelly Deters
4
Filling each coefficient location lets you and the grader know that you finished the problem rather than you left some blank because you weren’t done!
Place a “1” in any empty coefficient location
_____ __________2
How to Balance By Inspection:
Reactants Products
H
O
4
2 3
2
C 1 1
2
4
44
1 1CH4 + O2 _____ H2 O CO2+
Taken from Kelly Deters
Choosing the Order of Balancing
Save for laterElements that are uncombined
Save for laterElements that appear more than 1 time per side
StartElements that appear
only 1 time per side
StartElements in most
complicated molecules
How do you know what order to balance in?
Pb + PbO2 + H+ Pb2+ + H2O
To balance this equation, use the order: O, H, Pb
Taken from Kelly Deters
_____
How is Balancing Affected by Order?
What happens if we balance in the order determined in the last slide?
Reactants Products
H
Pb
1
2 1
2
O 2 1
4
2
_____ __________1 21 2Pb Pb+ O2 H2 O Pb2++H+_____4+
2
4
O, H, Pb
Taken from Kelly Deters
2
_____
What about a different order?
How is it different if we balance in a different order?
Reactants Products
O
Pb
2
2 1
1
H 1
2
2
_____ __________1 21 2Pb Pb+ O2 H2 O Pb2++H+_____2+
2 4
4
4
You’ll still get to the correct answer, but it will take longer and be more complicated!
H, O, Pb
Taken from Kelly Deters
Let’s Practice #1
Example:Balance the
following equation
__ HCl + __ Ca(OH)2 __ CaCl2 + __ H2O
Taken from Kelly Deters
Let’s Practice #1
Example:Balance the
following equation
__ HCl + __ Ca(OH)2 __ CaCl2 + __ H2O2 1 1 2
HOH
Did you see the “OH” polyatomic ion & change H2O to HOH?
Taken from Kelly Deters
Let’s Practice #2
Example:Balance the
following equation
__ H2 + __ O2 __ H2O
Taken from Kelly Deters
Let’s Practice #2
Example:Balance the
following equation
__ H2 + __ O2 __ H2O2 1 2
Taken from Kelly Deters
Let’s Practice #3
Example:Balance the
following equation
__ Fe + __ O2 ___ Fe2O3
Taken from Kelly Deters
Let’s Practice #3
Example:Balance the
following equation
__ Fe + __ O2 ___ Fe2O34 3 2
Homework
Pg. 181 # 6-9
Do Now
Balance the following equations:
__Cu +__AgNO3 -> __Cu(NO3)2 + __Ag
___NaClO3 --> ___NaCl + ___O2
Objectives
1. SWBAT define mole, representative particle, and molar mass.
2. SWBAT calculate the molar mass of substances.
Adopted from "Chemistry You Need to Know" by Kelly Deters
C.5 The Mole Concept
Definition:
Mole – SI unit for counting
Adopted from "Chemistry You Need to Know" by Kelly Deters
What is a counting unit?
You’re already familiar with one counting unit…a “dozen”
“Dozen” 12
A dozen doughnuts 12 doughnuts
A dozen books
A dozen cars
A dozen people
12 books
12 cars
12 people
A dozen = 12
Adopted from "Chemistry You Need to Know" by Kelly Deters
How big is a mole? Enough soft drink cans to cover the
surface of the earth to a depth of over 200 miles.
If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles.
If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.
Adopted from "Chemistry You Need to Know" by Kelly Deters
A Mole of ParticlesA Mole of Particles Contains 6.02 x 1023 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 1023 H2O molecules
1 mole NaCl= 6.02 x 1023 NaCl “molecules”
(technically, ionics are compounds not molecules so they are called formula units)
6.02 x 1023 Na+ ions and 6.02 x 1023 Cl– ions
Adopted from "Chemistry You Need to Know" by Kelly Deters
What does a “mole” count in?
A mole = 6.02 1023 (called Avogadro’s number)
“mole” 6.02 1023
1 mole of doughnuts 6.02 1023 doughnuts
1 mole of atoms
1 mole of molecules
6.02 1023 atoms
6.02 1023 molecules
6.02 1023 = 602,000,000,000,000,000,000,000
This means a 12 ounce bottle of water would have 19.7 “moles” of water…a much easier-to-work-with number!
Adopted from "Chemistry You Need to Know" by Kelly
Deters
Molar Mass
Adopted from "Chemistry You Need to Know" by Kelly Deters
Definition
Molar Mass – The mass for one mole of an atom or molecule.
Other terms commonly used for the same meaning:Molecular WeightMolecular MassFormula WeightFormula Mass
Adopted from "Chemistry You Need to Know" by Kelly Deters
Mass for 1 mole of atomsThe average atomic mass = grams for 1 mole
Element Mass
1 mole of carbon atoms 12.01 g
1 mole of oxygen atoms
1 mole of hydrogen atoms
16.00 g
1.01 g
Unit for molar mass: g/mole or g/mol
Average atomic mass is found on the periodic table
Adopted from "Chemistry You Need to Know" by Kelly Deters
Molar mass for molecules
The molar mass for a molecule = the sum of the molar masses of all the atoms
Adopted from "Chemistry You Need to Know" by Kelly Deters
Calculating a Molecule’s Mass
Count the number of each type of atom
Find the molar mass of each atom on the periodic table
Multiple the # of atoms molar mass for each atom
Find the sum of all the masses
1
2
3
4
To find the molar mass of a molecule:
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass
Example:Find the
molar mass for
CaBr2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass
Count the number of each type of atom1
Ca
Br
1
2
Example:Find the
molar mass for
CaBr2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass
Find the molar mass of each atom on the periodic table2
Ca
Br
1
2
40.08 g/mole
79.91 g/mole
Example:Find the
molar mass for
CaBr2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass
Multiple the # of atoms molar mass for each atom3
Ca
Br
1
2
40.08 g/mole
79.91 g/mole
Example:Find the
molar mass for
CaBr2
= 40.08 g/mole
= 159.82 g/mole
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass
Find the sum of all the masses4
Ca
Br
1
2
40.08 g/mole
79.91 g/mole
= 40.08 g/mole
= 159.82 g/mole+
199.90 g/mole
1 mole of CaBr2 molecules would have a mass of 199.90 g
Example:Find the
molar mass for
CaBr2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass & Parenthesis
Be sure to distribute the subscript outside the parenthesis to each element inside the parenthesis.
Example:Find the
molar mass for Sr(NO3)2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Molar Mass & Parenthesis
Be sure to distribute the subscript outside the parenthesis to each element inside the parenthesis.
1
6
87.62 g/mole
16.00 g/mole
= 87.62 g/mole
= 96.00 g/mole+
211.64 g/mole
1 mole of Sr(NO3)2 molecules would have a mass of 211.64 g
2 14.01 g/mole = 28.02 g/mole
Sr
N
O
Example:Find the
molar mass for Sr(NO3)2
Adopted from "Chemistry You Need to Know" by Kelly Deters
Let’s Practice #2
Example:Find the
molar mass for Al(OH)3
Adopted from "Chemistry You Need to Know" by Kelly Deters
Let’s Practice #2
Be sure to distribute the subscript outside the parenthesis to each element inside the parenthesis.
1
2
26.98 g/mole
1.01 g/mole
= 26.98 g/mole
= 2.02 g/mole+
61.00 g/mole
1 mole of Al(OH)3 molecules would have a mass of 61.00 g
2 16.00 g/mole = 32.00 g/mole
Al
O
H
Example:Find the
molar mass for Al(OH)3
Adopted from "Chemistry You Need to Know" by Kelly
Deters
Using Molar Mass in Conversions
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Moles to Grams
Example:How many grams are
in 1.25 moles of water?
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Moles to Grams
1.25 mol H2O = _______ g H2Omol H2O
g H2O18.02
1
22.53
When converting between grams and moles, the molar mass is needed
1 mole H2O molecules = 18.02 g
HO
21
1.01 g/mole16.00 g/mole
= 2.02 g/mole= 16.00 g/mole+
18.02 g/mole
Example:How many grams are
in 1.25 moles of water?
Adopted from "Chemistry You Need to Know" by Kelly Deters
Let’s Practice #3
Example:How many moles are in 25.5 g NaCl?
Adopted from "Chemistry You Need to Know" by Kelly Deters
Let’s Practice #3
25.5 g NaCl = _______ mole NaClg NaCl
mole NaCl1
58.44
0.44
1 mole NaCl molecules = 58.44 g
NaCl
11
22.99 g/mole35.45 g/mole
= 22.99 g/mole= 35.45 g/mole+
58.44 g/mole
Example:How many moles are in 25.5 g NaCl?
Adopted from "Chemistry You Need to Know" by Kelly Deters
Example: Grams to Molecules
Example:How many molecules
are in 25.5 g NaCl?
Adopted from "Chemistry You Need to Know" by Kelly Deters
25.5 g NaCl
Example: Grams to Molecules
= _________ molecules NaCl
g NaCl
mol NaCl1
58.44
2.63 1023
1 mol = 6.021023 molecules
1 moles NaCl molecules = 58.44 g
NaCl
11
22.99 g/mole35.45 g/mole
= 22.99 g/mole= 35.45 g/mole+
58.44 g/mole
mol NaCl
molecules NaCl6.021023
1
Example:How many molecules
are in 25.5 g NaCl?
Do Now
Solve the following problem: How many moles are in 6.7 g of NaCl?
A. Given: Unknown (attain):B. What is your conversion factor?C. Solve:
Objectives
SWBAT practice conversions between moles and grams
SWBAT practice conversions between moles and molecules
Adopted from "Chemistry You Need to Know" by Kelly Deters
Let’s Practice #4
Example:How many grams is a sample of 2.75 × 1024
molecules of SrCl2?
Adopted from "Chemistry You Need to Know" by Kelly Deters
2.75 × 1024 molecules SrCl2
Let’s Practice #4
= _________ g SrCl2
molecules SrCl2
mol SrCl21
6.02 × 1023
7.24
1 mol = 6.021023 molecules
1 moles SrCl2 molecules = 158.52 g
SrCl
12
87.62 g/mole35.45 g/mole
= 87.62 g/mole= 70.90 g/mole+
158.52 g/mole
mol SrCl2
g SrCl2158.52
1
Example:How many grams is a sample of 2.75 × 1024
molecules of SrCl2?
REMEMBER:
If you are going between moles and mass use MOLAR MASS.
1 mole molar mass (g)molar mass (g) 1 mole
If you are going between moles and molecules (atoms) use AVOGADROS NUMBER.
6.02 X 1023 molecules 1 mole . 1 mole 6.02 X 1023 molecules
Do Now
Solve the following problem: How many molecules are in 0.8 moles of NaCl?
A. Given: Unknown (attain):B. What is your conversion factor?C. Solve:
Objectives
SWBAT practice conversions between moles and grams
SWBAT practice conversions between moles and molecules
Adopted from "Chemistry You Need to Know" by Kelly Deters
THINK-PAIR-SHARE
1. How many moles are in 2.3 X 1024 molecules of NaCl?
2. How many moles are in 6.8 X 1026 molecules of CO2?
3. How many molecules are in 2.3 moles of HCl?
GRAMS to MOLECULES
How many molecules are in 4.6 grams of HCl?
Do Now
Solve the following problem: How many moles are in 2.8 g of HCl?
A. Given: Unknown (attain):B. What is your conversion factor?C. Solve:
Objective
1. SWBAT review problems where molar mass converts between moles and grams.
2. SWBAT determine molar relationships amount reactants and products in a chemical equation.
Steps to Solving Equations and Molar Relationships
1. Balance the equation. 2. State the GIVEN and what you
want to ATTAIN (UNKOWN) 3. Figure out conversions. 4. SOLVE!
WORKSHEET PROBLEM #1 MOLES TO MOLES
2Mg + O2 -> 2MgO
How many moles of Mg are needed to produce 6 moles of MgO?
How many moles of O2 are needed to produce 4 moles of MgO?
How many moles of MgO will be produced when 7 moles O2 enter the reaction?
WORKSHEET PROBLEM #1 MOLES TO MOLES to Grams
2H2O2 -> 2H2O + O2
How many grams of H2O2 are needed to produce 6 moles of O2?
DO NOw
For the following equation:
2Cu + O2 -> 2CuO
1. How many moles of Cu are needed to react with 15 moles O2?
2. How many moles of CuO produced when 11 moles Cu react with sufficient O2?
Objectives
SWBAT calculate moles of product and moles of reactants.
SWAT answer questions on molar mass, g to molecules, and stoichometry.
For the following reaction:
___C5H12 + ___O2 --> ___CO2 + ___H2O
If 10 moles of C5H12 enter the reaction, how many moles of H2O are produced?
If 13 moles CO2 are produced, how many moles O2 went in?
If 10 moles of C5H12 enter the reaction, how many grams of H2O are produced?
Think-Pair-Share
Pg. 166 #1-4
Do Now
2Cu + O2 -> 2CuO
1. How many moles of Cu are needed to react with 5.6 moles O2 ?
2. How many grams of Cu will be needed to react with 5.6 moles O2 ?
Objectives
1. SWBAT calculate percent compositions.
2. SWBAT explain why knowledge of percent compositions is important to the mining process.
Percent Composition
Percent by mass of each material found in a formula unit.
Ex. In Cu2S, it is 80% copper.
Determining Percent Composition
1. Find the molar mass of the formula unit.
2. Find the percentage by dividing the part by the whole and multiplying by 100.
Example
Let’s Try this one
Find the percent oxygen in the following formulas:CO2
C6H12O6
Think-Pair-Share
How is percent composition important when mining metals?
How is it important when selecting your metal for your coin?
Homework
Read 166-168 Pg. 168 #1-4
Do Now
What percent of oxygen is found in Calcium Nitrate? Ca(NO3)2
Objectives
SWBAT answer questions to help them review for their upcoming test on chapter 2.C
SWBAT retrieve copper from it’s ore and answer questions on the lab.
C.12. Conservation in the Community
Renewable Resources: replenished by natural processesEx. Water, air, soil, plants, animals
Nonrenewable Resources: cannot be readily replenished.Ex. Natural gas, coal, oil
Conserving Resources
Green Chemistry 4 Rs
RethinkingReusingReplacingRecycling