Chapter 3 Mass Relationships in Chemical Reactions.
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Transcript of Chapter 3 Mass Relationships in Chemical Reactions.
Chapter 3Mass Relationships in Chemical Reactions
Atomic Mass What is atomic
mass? Mass of an atom in
atomic mass units (AMU) 1 AMU is the mass of
1/12 of a carbon-12 atom
Also called atomic weight
Relative Atomic Mass What does the
relative atomic mass of an element represent?
Average mass of all known existing isotopes of that element
It is “unitless” Proportioned based
on abundance Ex. Carbon has a
mass of 12.011 which is an average of all of the carbon isotopes
Isotope ProportionsA certain sample of element Z contains 60% of 69Z and 40% of 71Z.
What is the relative atomic mass of element Z in this sample?
Isotope ProportionsChlorine exists as two isotopes, 35Cl and 37Cl. The relative atomic mass of chlorine is 35.45.
Calculate the percentage abundance of each isotope.
Molar Mass and NA
What unit is used to measure the number of atoms/molecules?
Moles (mol) – the number of atoms in 12 grams of a carbon-12 sample
1 mole = 6.02 x 1023
Avogadro's number (NA)
We use it like we would a pair (2), dozen (12), or a gross (144) to simplify our math because it is freaking huge
How Big Is A Mole?1. If you would distribute 1 mole of pennies among the
current population of the Earth, how much would everyone get?
2. How long would it take to spend this amount if you would spend $1,000/day?
3. How many people could you make from 1 mole of cells?
4. How long is 1 mole of seconds? 5. If we took a mole of regular 8.5 x 11 inch sheets of
paper and started laying them out side by side on the planet’s surface. What percentage of the Earth would be covered?
How Big Is A Mole? Answers1. $900 million dollars2. 2,500,000 years3. 10 billion4. 950,000 x age of the universe (14 billion
yrs)5. 100 %
…and it would be 17 million sheets thick
Molar Mass How is molar mass
different from relative atomic mass?
It is the mass of one mole of a substance
Abbreviated MM Same number as
atomic mass, but with different units Units: IB Units: g mol-1
Molar Mass What is the molar
mass (MM) of the following elements? Lithium Plutonium Bromine
6.94 239.05 79.91
Molar Mass How do we
determine the molar mass of a molecule?
What is the molar mass of water?
Add up the molar masses of each element within the molecule
H2O MM = 2(H) + 1(O) MM = 2(1.01) + 1(16.00 ) MM = 18.02
Molecular Vs. Molar What is the
difference between atomic, molecular and molar mass?
Different units for different purposes
Atomic/Molecular Mass AMU’s
Molar Mass
Can be used interchangeably
Molar Mass What is the molar
mass of each of the following species: KBr FeCl3 Sodium Hydroxide Lead (II) Oxide
119.01
162.20
40.00
223.19
Navigating How can we
navigate between mass (m), moles (n) and the number of atoms, molecules or particles?
We use molar mass (MM) and Avogadro's number (NA)
Double Circles
Double Triangles
NAAvogadro's number
mmass
nmoles
MMmolar mass
nmoles
Nnumber
Mass-Mole Conversions1. How many moles in 28 grams of CO2 ?
2. What is the mass of 5 moles of Fe2O3 ?
3. Find the number of moles of argon in 452 g of argon.
4. Find the grams in 1.26 x 10-4 mol of HC2H3O2.
5. Find the mass in 2.6 mol of lithium bromide.
Mole-Number Conversions1. How many moles of magnesium is 3.01 x 1022
atoms of magnesium?
2. How many molecules are there in 4.00 moles of glucose, C6H12O6?
3. How many moles are 1.20 x 1025 atoms of phosphorous?
4. How many atoms are in 0.750 moles of zinc?
5. How many oxygen atoms are in 0.400 moles of N2O5?
To the right, To the right How many atoms
are in 20.0 grams of gold?
Mass 20.0 g Divide by molar mass
to get to moles 0.102 moles
Multiply by Avogadro's number to get to atoms 6.14E22 Au atoms
To the left, To the left What is the mass of
1.00E24 carbon atoms?
Number 1.00E24 atoms
Divide by Avogadro's number to get to moles 1.66 moles
Multiply by molar mass to get mass 19.9 grams
Combined1. Find the mass in grams of 2.00 x 1022
molecules of diatomic fluorine.
2. Find the number of molecules in 60.0 g of dinitrogen monoxide.
3. How many molecules are in 5 mg of aspartame, C14H18N2O5?
4. Calculate the mass, in grams, of 6.69x1021 ethane (C2H6) molecules.
5. Urea [(NH2)2CO] is used for fertilizer and many other things. Calculate the number of N,C,O and H atoms in 1.68 x 104 grams of urea.
6. The density of water is 1.00 at 4°C. How many water molecules are present in 2.56 mL of water at this temperature?
Combined
PRELAB 1Gum
PRELAB 1Sugar in Chewing Gum How can we test
for the mass of sugar in chewing gum?
PRELAB 1Sugar in Chewing Gum
In your notebook, please calculate the following with proper uncertainties, sig figs and units.1. Experimental mass of sugar in the gum with
the correct uncertainties
2. Percent mass of sugar in your piece of gum
3. Percent error =
PRELAB 1Sugar in Chewing Gum Compare and contrast your measured
percentage of sugar, and the actual percentage from the nutrition label for the brand of gum that you used.
What are some possible reasons for any differences in these values, and how you might increase the accuracy of your data collection?
PRELAB 1Sugar in Chewing Gum
What mathematical relationship/formula did you use to determine percent by
mass? Why?
If you were given one molecule of sucrose, C6H12O6, what information do you think you would need to figure out the percent mass
of carbon? Why?
Percent Composition What is percent
composition?
What two pieces of info do we need?
Relative measure of the mass of each different element present in the compound
x 100
Mass of the element and the compound
Percent Composition How do we
calculate it?1. Calculate the mass
of the compound
2. Calculate the mass of each element
Percent Composition What is the
percent mass of hydrogen in water?
2 hydrogens 2(1.01) = 2.02 g/mol
Water is H2O 18.02 g/mol
2.02/18.02 x100 = 11.2% (tenths place)
Percent Composition Calculate the percent composition of
oxygen in sodium sulfate. Na2SO4 142.04 g/mol 4 oxygens 4(16.00) = 64.00 g/mol (64.00/142.04) x 100 = 45.1%
Percent Composition Tartrazine, or yellow dye # 5, is
commonly found in many foods. Its molecular formula is C16H9N4Na3O9S2 . What is the percent composition of Carbon and Sulfur? The molar mass of Tartrazine is 534.4 g/mol.
Working in Reverse If we start with
%’s, what can that possibly lead us to?
Working the formula in reverse and using mole ratios, we can get the empirical and possibly the molecular formula
Determination of the Empirical Formula
How do we determine it?
1. Assume that you have 100% of the element and set equal to mass
2. Divide each element by its molar mass
3. Divide each by the smallest amount of moles
4. If numbers aren’t close to whole, multiply all of them by a coefficient
Butane’s Empirical Formula Butane is made up of only carbon and
hydrogen. If hydrogen makes up 17.34% of butane’s mass and carbon the remaining 82.66%, what is the empirical formula of butane? C2H5
What is the molecular formula for butane if its molecular mass is 58.14 g/mol? Multiply each subscript by 2 C4H10
Determine the Empirical Formula Determine the empirical formula of a
compound having the following percent composition by mass… K: 24.75% Mn: 34.77% O: 40.51%Empirical Formula: KMnO4
What is the molecular formula if its molecular mass is 158.04 g/mol?
ANSWER: KMnO4 (potassium permanganate)
Chemical Reactions and Equations
What is the difference between a chemical reaction and equation?
A chemical reaction is the process of making a new substance(s) Ex. Iron oxidizing
A chemical equation is a symbolic representation of the reaction 4Fe + 3O2 → 2Fe2O3
Chemical Reactions and Equations
How do we read a chemical equation?
4Fe(s) + 3O2(g) → 2Fe2O3(s) Reactants (left) Products (right) → Goes in one direction ↔ Reversible reaction Coefficients represent
the mole ratios Notations (s, l, g, aq)
represent phases/states Conservation of mass Balanced
Chemical Reactions and Equations
What is a balanced equation?
The number of atoms on the left has to equal the number on the right
Use coefficients to balance them
Unbalanced: CH4 + O2 → CO2 + H2O
Balanced:
Chemical Reactions and Equations How do we balance the equations? KClO3 → KCl + O2 2KClO3 → 2KCl + 3O2
Al + O2 → Al2O3
4Al + 3O2 → 2Al2O3
C2H6 + O2 → CO2 + H2O 2C2H6 + 7O2 → 4CO2 + 6H2O
Chemical Reactions and EquationsBalance the following chemical equations: K2CO3 + HCl KCl + H2O + CO2
K2CO3 + 2HCl 2KCl + H2O + CO2
CaCO3 + HNO3 Ca(NO3)2 + H2O + CO2
CaCO3 + 2HNO3 Ca(NO3)2 + H2O + CO2
Pb(NO3)2 + NaI PbI2 + NaNO3
Pb(NO3)2 + 2NaI PbI2 + 2NaNO3
Al2(SO4)3 + NaOH Al(OH)3 + Na2SO4
Al2(SO4)3 + 6NaOH 2Al(OH)3 + 3Na2SO4
Amounts of Reactants and Products
What is stoichiometry? The study of any numerical observation within a chemical reaction
Using the mole method to determine how much reactant is needed (or product created) based on the number of moles
Amounts of Reactants and Products
What can be said about the reaction: H2 + O2 → H2O
Reactants: Hydrogen and Oxygen
Products: Water Unbalanced Balanced: 2H2 + O2→2H2O Proportion: 2 moles of
hydrogen and 1 mole of oxygen create 2 moles of water
Amounts of Reactants and Products
How many moles of water should be formed with 8 moles of oxygen?
What happens when our measurements are not in moles?
1:2 Ratio 8 moles of oxygen is
equivalent to 16 moles of water
Convert them into moles before starting using molar mass
Amounts of Reactants and Products
I have the formula: Mg + HCl → MgCl2 + H2
What is the mass of MgCl2 that is formed when 20.0 g of HCl reacts with Mg? 1. Balance it
Mg + 2HCl → MgCl2 + H2
2. Convert into moles (20.0 g)/(36.45 g/mol) = 0.549 mol HCl
3. Use the mole ratio method 2:1 ratio → 0.275 mol MgCl2
4. Convert back into mass 0.275 mol MgCl2 → 26.2 g
Amounts of Reactants and Products
What mass of silver nitrate as a solution in water would need to be added to 5.0 g of sodium chloride to ensure a complete precipitation of the chloride?
AgNO3(aq)+ NaCl (aq) AgCl(s) + NaNO3(aq)
Amounts of Reactants and Products
What mass of barium sulfate would be produced from 10.0 g of barium chloride in the following reaction?
BaCl2 + H2SO4 BaSO4 + HCl
Balanced: BaCl2 + H2SO4 BaSO4 + 2HCl
Amounts of Reactants and Products
What volume of ammonia gas would be needed to produce 40. g of ammonium nitrate in the following reaction.
NH3 (g) + HNO3 (aq) NH4NO3 (aq)
Amounts of Reactants and Products
In a fermentation reaction, glucose is converted to alcohol and carbon dioxide according to the following equation. What mass of alcohol and carbon dioxide would be produced from 10. g of glucose?
C6H12O6 C2H5OH + CO2
Balanced: C6H12O6 2C2H5OH + 2CO2
Amounts of Reactants and Products
What is the difference between theoretical and actual yield?
What is its purpose?
Theoretical is the predicted amount of product via stoichiometry
Actual is how much product you obtained experimentally
To determine the efficiency of the procedure and/or experiment
Reaction Yield
Reaction Yield What is the % yield
of CO2 if you started with 10.00 g of O2 obtained 22.53 g of CO2?
CO + O2 CO2
Balanced: 2CO + O2 → 2CO2
100% ltheoretica
actualyield
Limiting Reagent
What is a limiting reagent?
The reactant that is depleted first during a reaction is limiting
Prevents a reaction from achieving 100% yield
Any reactants remaining after the reaction completes are called excess reagents i.e. anything in excess
cannot be a limiting reagent
Limiting Reagent 124 g of aluminum react with 601 g of iron (III)
oxide. Calculate the mass of Al2O3 formed.
Al + Fe2O3 → Al2O3 + Fe
2Al + Fe2O3 → Al2O3 + 2Fe
1. Balance!2. Determine the number of moles of each reactant.3. Divide by the molar coefficient to determine the
limiting reagent4. Use that number of moles to determine the
amount produced using proper stoichiometry
Limiting Reagent Table
Reaction 2Al Fe2O3 Al2O3 2Fe
Molar Mass (g/mol)
Initial Mass (g)
Initial Moles (mol)
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent Table
Reaction 2Al Fe2O3 Al2O3 2Fe
Molar Mass (g/mol)
26.98 159.70 101.96 55.85
Initial Mass (g) 124 601 0 0
Initial Moles (mol)
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent TableReaction 2Al Fe2O3 Al2O3 2Fe
Molar Mass (g/mol)
26.98 159.70 101.96 55.85
Initial Mass (g) 124 601 0 0
Initial Moles (mol) 4.60 3.76 0 0
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent TableReaction 2Al Fe2O3 Al2O3 2Fe
Molar Mass (g/mol)
26.98 159.70 101.96 55.85
Initial Mass (g) 124 601 0 0
Initial Moles (mol) 4.60 3.76 0 0
Limiting Reagent (mol)
2.30 3.76 0 0
Final Moles (mol)
Final Mass (g)
Limiting Reagent Table
Reaction 2Al Fe2O3 Al2O3 2Fe
Molar Mass (g/mol) 26.98 159.70 101.96 55.85
Initial Mass (g) 124 601 0 0
Initial Moles (mol) 4.60 3.76 0 0
Limiting Reagent (mol)
2.30 3.76 0 0
Final Moles (mol) 4.60 2.30 2.30 4.60
Final Mass (g) 124 367 235 257
Note: The mass of reactants equals the approximate mass of the products
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2OReaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol)
Initial Mass (g)
Initial Moles (mol)
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2OReaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25 48.2 0 0 0
Initial Moles (mol)
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
Reaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25 48.2 0 0 0
Initial Moles (mol) 0.5435 1.32 0 0 0
Limiting Reagent (mol)
Final Moles (mol)
Final Mass (g)
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2OReaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25 48.2 0 0 0
Initial Moles (mol) 0.5435 1.32 0 0 0
Limiting Reagent (mol)
0.5435 0.330
0 0 0
Final Moles (mol)
Final Mass (g)
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2OReaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25 48.2 0 0 0
Initial Moles (mol) 0.5435 1.32 0 0 0
Limiting Reagent (mol)
0.5435 0.330
0 0 0
Final Moles (mol) 0.330 1.32 0.330 0.330 0.660
Final Mass (g)
Limiting Reagent How much chlorine is produced in the following reaction
when 47.25 g of manganese (IV) oxide reacts with 48.2 g of hydrochloric acid?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2OReaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25 48.2 0 0 0
Initial Moles (mol) 0.5435 1.32 0 0 0
Limiting Reagent (mol)
0.5435 0.330
0 0 0
Final Moles (mol) 0.330 1.32 0.330 0.330 0.660
Final Mass (g) 28.7 48.1 41.5 23.4 11.9
Excess Reagent If you started with 47.25 g, how much manganese (IV)
oxide is left in excess after the reaction is completed?
47.25 – 28.7 = 18.6 g of MgO2 excess
Reaction MnO2 4HCl MnCl2 Cl2 2H2O
Molar Mass (g/mol) 86.93 36.46 125.83 70.90 18.02
Initial Mass (g) 47.25
48.2 0 0 0
Initial Moles (mol) 0.5435 1.32 0 0 0
Limiting Reagent (mol)
0.5435 0.330 0 0 0
Final Moles (mol) 0.330 1.32 0.330 0.330 0.660
Final Mass (g) 28.7 48.1 41.5 23.4 11.9
Limiting Reagent
Limiting Reagent
Practice Problem – pg. 93
Limiting Reagent
Practice Problem – pg. 95
Limiting Reagent
Practice Problem – pg. 96
Reaction Yield