Transcript Stoichiometry

Stoichiometry:
Calculations with Chemical
Formulas and Equations
Stoichiometry
EVIDENCE OF A CHEMICAL REACTION
•A gas is released.
•An insoluble substance (called a precipitate) is
produced.
•A permanent color change is observed.
•Changes in energy.
Heat, light, sound, and electrical.
Exothermic reaction: releases heat,light and
sound.
Endothermic reaction: absorbs heat and light.
•pH change
•Odor given off
Stoichiometry
EVIDENCE OF A CHEMICAL REACTION USING
YOUR SENSES:
Sight- Change in color, formation of solid,
formation of gasses (bubbles), light emission
Hearing- reaction leads to a popping noise,
fizzes
Smell- pungent odor, change in smell
Touch- heat absorption and emission
Stoichiometry
Law of Conservation of Mass
“We may lay it down as an
incontestable axiom that, in all
the operations of art and nature,
nothing is created; an equal
amount of matter exists both
before and after the experiment.
Upon this principle, the whole art
of performing chemical
experiments depends.”
--Antoine Lavoisier, 1789
Stoichiometry
Chemical Equations
Concise representations of chemical
reactions
Stoichiometry
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g)
CO2 (g) + 2 H2O (g)
Stoichiometry
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g)
Reactants appear on the
left side of the equation.
CO2 (g) + 2 H2O (g)
Stoichiometry
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g)
Products appear on the
right side of the equation.
CO2 (g) + 2 H2O (g)
Stoichiometry
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g)
CO2 (g) + 2 H2O (g)
The states of the reactants and products
are written in parentheses to the right of
each compound.
Stoichiometry
Anatomy of a Chemical Equation
CH4 (g) + 2 O2 (g)
Coefficients are inserted to
balance the equation.
CO2 (g) + 2 H2O (g)
Stoichiometry
Subscripts and Coefficients Give
Different Information
• Subscripts tell the number of atoms of
each element in a molecule
Stoichiometry
Subscripts and Coefficients Give
Different Information
• Subscripts tell the number of atoms of
each element in a molecule
• Coefficients tell the number of
molecules
Stoichiometry
Coefficients in Chemical Reactions
• Coefficients tell how many molecules
or atoms there are.
• Coefficients are numbers placed in
front of each molecule or atom and
are used to balance equations.
Stoichiometry
Conservation of Mass and Atoms
• Law of Conservation of Matter:
• Mass is neither created or destroyed
in chemical reactions.
– Lavoisier (1743-1794) proved this.
• The number and kinds of atoms
present in the products is the same
number and kind of atoms present in
the reactants.
– The atoms just rearrange.
Stoichiometry
Writing and Balancing Equations
• Determine the reactants and products.
• Write the equation.
– Use the correct formulas for each compound—
watch for the diatomics; those that end in
–ine and –gen. (H2, N2, O2, F2, Cl2, Br2, I2, At2).
• Balance the equation (same # and kind of
elements on both sides of the arrow).
Stoichiometry
Balancing Examples
• Solid copper(II) oxide reacts with
hydrogen gas to form solid copper and
liquid water.
CuO (s) + H2 (g) ---> Cu (s) + H2O (l)
• Aluminum metal reacts with oxygen gas
to form solid aluminum oxide.
Al (s) + O2 (g) ---> Al2O3 (s)
Stoichiometry
Balancing Examples
• When balancing an equation, ONLY the
coefficients can be changed.
• NEVER change the subscripts.
• For example: 3H2O
3 is the coefficient.
2 and 1 are the subscripts.
• Changing the subscripts changes the
compound.
H2O2  is not water but hydrogen peroxide.
Stoichiometry
HELPFUL HINTS
•
Keep polyatomic ions together as a
unit if they show up on both sides of
the equation.
-- NO3-1 , C2H3O2-1 , NH4+1 , ….
-- Ca(NO3)2 + NaCl ---> CaCl2 + NaNO3
•
Save H and O until last.
-- They will tend to balance out together
with the H2O.
Stoichiometry
Example
Aluminum sulfide reacts with water to
produce aluminum hydroxide and
hydrogen sulfide.
Al2S3 + H2O --> Al(OH)3 + H2S
What should we look for immediately?
Save O and H for last - there is water.
Al2S3 + H2O ---> 2 Al(OH)3 + H2S
Al2S3 + H2O ---> 2 Al(OH)3 + 3 H2S
The Al and S are balanced - now  H & O.
Al2S3 + 6 H2O ------> 2 Al(OH)3 + 3 H2S
Stoichiometry
Balance The Following Equations
•
•
•
•
•
•
•
•
•
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•
Al + S8
Al2S3
16 Al + 3 S8
8 Al2S3
CO + O2
CO2
2 CO + O2
2 CO2
C2H4 + O2
CO2 + H2O
C2H4 + 3 O2
2 CO2 + 2 H2O
Pb(NO3)2 + NaCl
PbCl2 + NaNO3
Pb(NO3)2 + 2 NaCl
PbCl2 + 2 NaNO3
Mg2C3 + H2O
Mg(OH)2 + C3H4
Mg2C3 + 4 H2O
2 Mg(OH)2 + C3H4
Ca(OH)2 + HBr
CaBr2 + H2O
Ca(OH)2 + 2 HBr
CaBr2 + 2 H2O
Stoichiometry
Reaction
Types
Stoichiometry
Combination or (Synthesis)
Reactions
• Two or more
substances
react to form
one product
• Examples:
N2 (g) + 3 H2 (g)  2 NH3 (g)
C3H6 (g) + Br2 (l)  C3H6Br2 (l)
2 Mg (s) + O2 (g)  2 MgO (s)
Stoichiometry
2 Mg (s) + O2 (g)  2 MgO (s)
Stoichiometry
Decomposition Reactions
• One substance breaks
down into two or more
substances
• Examples:
CaCO3 (s)  CaO (s) + CO2 (g)
2 KClO3 (s)  2 KCl (s) + O2 (g)
2 NaN3 (s)  2 Na (s) + 3 N2 (g)
Stoichiometry
Combustion Reactions
• Rapid reactions that
produce a flame
• Most often involve
hydrocarbons
reacting with oxygen
in the air
• Examples:
CH4 (g) + 2 O2 (g)  CO2 (g) + 2 H2O (g)
C3H8 (g) + 5 O2 (g)  3 CO2 (g) + 4 H2O (g)
Stoichiometry
Formula
Weights
Stoichiometry
Formula Weight (FW)
• Sum of the atomic weights for the atoms
in a chemical formula
• So, the formula weight of calcium
chloride, CaCl2, would be
Ca: 1(40.1 amu)
+ Cl: 2(35.5 amu)
111.1 amu
• These are generally reported for ionic
compounds
Stoichiometry
Molecular Weight (MW)
• Sum of the atomic weights of the atoms
in a molecule
• For the molecule ethane, C2H6, the
molecular weight would be
C: 2(12.0 amu)
+ H: 6(1.0 amu)
30.0 amu
Stoichiometry
Percent Composition
One can find the percentage of the mass
of a compound that comes from each of
the elements in the compound by using
this equation:
(number of atoms)(atomic weight)
% element =
(FW of the compound)
x 100
Stoichiometry
Percent Composition
So the percentage of carbon in ethane
is…
(2)(12.0 amu)
%C =
(30.0 amu)
24.0 amu
x 100
=
30.0 amu
= 80.0%
Stoichiometry
Moles
Stoichiometry
Avogadro’s Number
• 6.02 x 1023
• 1 mole of 12C has a
mass of 12 g
Stoichiometry
The Mole—How big is
6.022 x 1023;
Avogadro ’s number?
602,200,000,000,000,000,000,000
Stoichiometry
It would take 10 billion chickens
laying 10 eggs per day more
than 10 billion years to lay a
mole of eggs.
Stoichiometry
Avogadro's number of inches
is 1,616,434 light years, or
across our galaxy and back 8
times.
Stoichiometry
Avogadro's number of seconds
is about 19 quadrillion years!
That is 4,240,666 times the age
of the earth, or 954,150 times
the age of the universe itself.
Stoichiometry
Avogadro's number of
kilograms is just over 20 times
the mass of the earth.
Stoichiometry
Avogadro's number of cents
could repay the United States
National Debt 86 million times.
Stoichiometry
Molar Mass
• By definition, these are the mass of 1
mol of a substance (i.e., g/mol)
– The molar mass of an element is the mass
number for the element that we find on the
periodic table
– The formula weight (in amu’s) will be the
same number as the molar mass (in g/mol)
Stoichiometry
Using Moles
Moles provide a bridge from the molecular scale
to the real-world scale
Stoichiometry
Mole Relationships
• One mole of atoms, ions, or molecules contains
Avogadro’s number of those particles
• One mole of molecules or formula units contains
Avogadro’s number times the number of atoms or
ions of each element in the compound
Stoichiometry
Finding
Empirical
Formulas
Stoichiometry
Calculating Empirical Formulas
One can calculate the empirical formula from
the percent composition
Stoichiometry
Calculating Empirical Formulas
The compound para-aminobenzoic acid (you may have
seen it listed as PABA on your bottle of sunscreen) is
composed of carbon (61.31%), hydrogen (5.14%),
nitrogen (10.21%), and oxygen (23.33%). Find the
empirical formula of PABA.
Stoichiometry
Calculating Empirical Formulas
Assuming 100.00 g of para-aminobenzoic acid,
C:
H:
N:
O:
1 mol
12.01 g
1 mol
5.14 g x
1.01 g
1 mol
10.21 g x
14.01 g
1 mol
23.33 g x
16.00 g
61.31 g x
= 5.105 mol C
= 5.09 mol H
= 0.7288 mol N
= 1.456 mol O
Stoichiometry
Calculating Empirical Formulas
Calculate the mole ratio by dividing by the smallest number
of moles:
C:
5.105 mol
0.7288 mol
= 7.005  7
H:
5.09 mol
0.7288 mol
= 6.984  7
N:
0.7288 mol
0.7288 mol
= 1.000
O:
1.458 mol
0.7288 mol
= 2.001  2
Stoichiometry
Calculating Empirical Formulas
These are the subscripts for the empirical formula:
C7H7NO2
Stoichiometry
Combustion Analysis
• Compounds containing C, H and O are routinely
analyzed through combustion in a chamber like this
– C is determined from the mass of CO2 produced
– H is determined from the mass of H2O produced
– O is determined by difference after the C and H have been
determined
Stoichiometry
Elemental Analyses
Compounds
containing other
elements are
analyzed using
methods analogous
to those used for C,
H and O
Stoichiometry
Stoichiometric Calculations
The coefficients in the balanced equation give
the ratio of moles of reactants and products
Stoichiometry
Stoichiometric Calculations
From the mass of
Substance A you can
use the ratio of the
coefficients of A and B
to calculate the mass
of Substance B
formed (if it’s a
product) or used (if
it’s a reactant)
Stoichiometry
Stoichiometric Calculations
C6H12O6 + 6 O2  6 CO2 + 6 H2O
Starting with 1.00 g of C6H12O6…
we calculate the moles of C6H12O6…
use the coefficients to find the moles of H2O…
and then turn the moles of water to grams
Stoichiometry
Limiting
Reactants
Stoichiometry
How Many Cookies Can I Make?
• You can make cookies
until you run out of one
of the ingredients
• Once this family runs
out of sugar, they will
stop making cookies
(at least any cookies
you would want to eat)
Stoichiometry
How Many Cookies Can I Make?
• In this example the
sugar would be the
limiting reactant,
because it will limit the
amount of cookies you
can make
Stoichiometry
Limiting Reactants
The limiting reactant
is the reactant
present in the
smallest
stoichiometric
amount
Stoichiometry
Limiting Reactants
• The limiting reactant is the reactant present in
the smallest stoichiometric amount
– In other words, it’s the reactant you’ll run out of first (in
this case, the H2)
Stoichiometry
Limiting Reactants
In the example below, the O2 would be the
excess reagent
Stoichiometry
Theoretical Yield
• The theoretical yield is the amount of
product that can be made
– In other words it’s the amount of product
possible as calculated through the
stoichiometry problem
• This is different from the actual yield,
the amount one actually produces and
measures
Stoichiometry
Percent Yield
A comparison of the amount actually
obtained to the amount it was possible
to make
Actual Yield
Percent Yield =
Theoretical Yield
x 100
Stoichiometry