Title: The Basics of Stoichiometry and Mole Calculations
1The Basics of Stoichiometry and Mole Calculations
- References and Resources
- Our TB Ch. 3 of Chemistry The central Science
AP version (10th edition) - Powerpoint and in-class work
- POGIL activities
- Online resources for our TB (in particular
Practice Quiz and e-book) - Concept map for Stoichiometry and problem solving
(handout) - Video lectures from chem guy (see next page)
- Chem tours from ch. 3 of the W.W. Norton online
book by Gilbert - http//www.wwnorton.com/college/chemistry/gilbert2
/contents/ch03/studyplan.asp - Some figures and examples in this PPT file have
been taken from Melissa Brophys presentation at
http//teacherweb.com/TX/McNeilHS/brophy/photo2.a
spx
2Resources Video lectures for Chemistry
- Chemguy videos (google AP chemistry and chemguy
videos use in sequence) - (good, short, video lectures that are
appropriate for regular, honors, or AP chemistry) - chem Guy video for mole 1 http//www.youtube.com
/watch?vxiVweBpjXJoplaynext1videoskHh8a0fILuY
featuremfu_in_order - Mole 2 chem guy http//www.youtube.com/watch?vxq
w2BWdKl1QfeaturePlayListpC09489B20AE215DFplay
next1playnext_fromPLindex19 - Mole 3 (Junior)
- http//www.youtube.com/watch?vO7qjYRYxksofeature
PlayListpC09489B20AE215DFplaynext1playnext_f
romPLindex20 - Â
- Stoichiometry video with worked example for
predicting amount of product from 2.6 mol of one
of reactant see http//www.youtube.com/watch?v-
W9-sNfM5Xofeaturerelated - Empirical formula for AP chem with chem. Guy
http//www.youtube.com/watch?vfFXtX_8NgsQfeature
related
3The Basics of Stoichiometry and Mole
Calculations
- Reading and writing chemical equations
- Balancing Equations
- Types of reactions
- Formula Weights
- Formula Weights and Molar Masses
- Percent composition
- Avagadros Number
- Mole calculations
- Solving problems using dimensional analysis using
(1) Avagadros number, (2) GFM, or (3) mole
ratios from coefficients of balanced equations - Determining Empirical formulas and Molecular
formulas - Limiting reagents(reactants)
4Chemical Equations
- Symbolic representations or descriptions of
chemical reactions - Meaning of the symbols, subscripts, parenthesis,
signs, arrows, co-efficients, states of matter,
etc. Vocab. terms reactants, products,
catalyst, reaction conditions , etc. - Use of particle diagrams (to represent)
- Conservation of Mass
- Resources POGIL activity Chemical Reaction
Equations (To Do)
5Reading Balanced Chemical Equations
- Molecules
- Particle diagrams
- Mass (amu)
- Amount (mol)
- Mass (g)
6Balancing Equations
- Objective find the smallest whole number ratio
of coefficients for reactants and products that
respects the law of conservation of mass. - How?
- Trial and error to some extent
- Can Not change subscripts in chemical formulas
- but you Can change co-efficients in front of
the formulas - Start by balancing those elements that occur in
the fewest chemical formulas - Move back and forth checking the atom count each
time a co-efficient is changed
7Practice Balancing Equations
- (example of a decomposition reaction that is used
in air bags in cars)
8Practice Balancing Equations (Index card
activity to hand in)
- (example of a combustion reaction)
- (Hint Start with the element that occurs in the
fewest chemical formulas)
9Formula Weights
- Calculating formula weights in amu using chemical
formula and the atomic masses from the periodic
table - Ex NaCl
- One formula unit of NaCl has a mass of ______amu
- Ex C6H12O6 (glucose)
- One molecule of glucose has a mass of ______amu
- Atomic masses of atoms, molecules and formula
unit - Atoms
- Ex Au (gold)
- One atom of Au has a mass of __________amu
10Percent Composition
- What is the percent carbon in C5H8NO4 (the
glutamic acid used to make MSG monosodium
glutamate), a compound used to flavor foods and
tenderize meats? -
11Percent Composition
- What is the percent carbon in C5H8NO4?
- Step 1 First calculate the Formula weight for
the compound (FW for C5H8NO4 is ________amu) -
- Step 2 composition (mass of part mass of
whole) X 100 - or
- element ( atoms of that element)(atomic
weight of the element) x 100 - Formula weight of the compound
-
12What is the carbon in MSG?
- Step 1 FW for C5H8NO4 is ________amu
-
- C
- H
- N
- O
13 Composition of Carbon in C5H8NO4
- Step 2 C (mass of part mass of whole) X
100 - or
- element ( atoms of element)(atomic weight of
the element) x 100 - Formula weight of the compound
- Answer?
14Percent Composition
- What is the percent carbon in C5H8NO4 (the
glutamic acid used to make MSG monosodium
glutamate), a compound used to flavor foods and
tenderize meats? - a) 8.22 C
- b) 24.3 C
- c) 41.1 C
15Avagadros number and The Mole
6.02 x 1023
602,000,000,000,000,000,000,000
16The Mole
- A counting unit
- Similar to a dozen, except instead of 12, its
602 billion trillion 602,000,000,000,000,000,000,0
00 - 6.02 X 1023 (in scientific notation)
- This number is named in honor of Amedeo _________
(1776 1856), who studied quantities of gases
and discovered that no matter what the gas was,
there were the same number of molecules present
17How big of a unit is a mole?
- 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.
18The Mole (abbreviated as mol)
- 1 dozen cookies 12 cookies
- 1 mole of cookies 6.02 X 1023 cookies
- 1 dozen cars 12 cars
- 1 mole of cars 6.02 X 1023 cars
- 1 dozen Al atoms 12 Al atoms
- 1 mole of Al atoms 6.02 X 1023 atoms
- Note that the NUMBER is always the same, but the
MASS is very different!
19A Mole of Particles Contains 6.02 x 1023
particles
- 6.02 x 1023 C atoms
- 6.02 x 1023 H2O molecules
- 6.02 x 1023 NaCl formula units
- (technically, ionic compounds are not molecules
so they are called formula units) - 6.02 x 1023 Na ions and
- 6.02 x 1023 Cl ions
1 mole C 1 mole H2O 1 mole NaCl
20Avogadros Number as Conversion Factor
- 6.02 x 1023 particles
- 1 mole
- or
- 1 mole
- 6.02 x 1023 particles
- Note that a particle could be an atom OR a
molecule!
21Learning Check
- 1. Number of atoms in 0.500 mole of Al
- a) 500 Al atoms
- b) 6.02 x 1023 Al atoms
- c) 3.01 x 1023 Al atoms
- 2.Number of moles of S in 1.8 x 1024 S atoms
- a) 1.0 mole S atoms
- b) 3.0 mole S atoms
- c) 1.1 x 1048 mole S atoms
-
22Practice Problems with /without using your
calculator
- How many hydrogen atoms are in 2.5 moles of
water? (Analyze, plan, solve, check)
23Molar Mass or Gram-Formula Mass (GFM)
- The Mass of 1 mole (in grams)
- Equal to the numerical value of the average
atomic mass (get from periodic table) - 1 mole of C atoms 12.0 g
- 1 mole of Mg atoms 24.3 g
- 1 mole of Cu atoms 63.5 g
24Other Names Related to Molar Mass or Gram-Formula
Mass (GFM)
- Molecular Mass/Molecular Weight If you have a
single molecule, mass is measured in amus
instead of grams. But, the molecular mass/weight
is the same numerical value as 1 mole of
molecules. Only the units are different. (This
is the beauty of Avogadros Number!) - Formula Mass/Formula Weight Same goes for
compounds. But again, the numerical value is the
same. Only the units are different. - THE POINT You may hear all of these terms which
mean the SAME NUMBER just different units
25Learning Check!
- Find the molar mass or gram-formula mass
(usually we round to the tenths place)
79.9 g/mole
- 1 mole of Br atoms
- 1 mole of Sn atoms
118.7 g/mole
26Practice Problems use mole road map or concept
map to help you solve
- How many atoms of copper are there in a 3 gram
sample of copper? - (Interconverting mass and numbers of particles)
27Problems involving Empirical Formulas and
Molecular Formulas
- Resources
- PPT
- POGIL
- Practice problems (in-class, chapter problem set,
online practice quiz questions)
28Chemical Formulas of Compounds
- Formulas give the relative numbers of atoms or
moles of each element in a formula unit - always
a whole number ratio (the law of definite
proportions). - NO2 2 atoms of O for every 1 atom of N
-
- 1 mole of NO2 2 mol of O atoms to every 1 mol
of N atoms - If we know, or can determine, the relative number
of moles of each element in a compound, we can
determine a formula for the compound.
29Types of Formulas
- Empirical Formula
- The formula of a compound that expresses the
smallest whole number ratio of the atoms present. - Ionic formula are always empirical formula
- Molecular Formula
- The formula that states the actual number of
each kind of atom found in one molecule of the
compound.
30To obtain an Empirical Formula
- 1. Determine the mass in grams of each element
present, if necessary. - 2. Calculate the number of moles of each
element. - 3. Divide each by the smallest number of moles to
obtain the simplest whole number ratio. - If whole numbers are not obtained in step 3),
multiply through by the smallest number that will
give all whole numbers - Be careful! Do not round off numbers
prematurely
31- A sample of a brown gas, a major air pollutant,
is found to contain 2.34 g N and 5.34g O.
Determine a formula for this substance. - require mole ratios so convert grams to moles
- moles of N 2.34g of N 0.167 moles
of N - 14.01 g/mole
- moles of O 5.34 g 0.334
moles of O - 16.00 g/mole
- Empirical Formula
32Calculation of the Molecular Formula
- A compound has an empirical formula of NO2. The
colourless liquid, used in rocket engines has a
molar mass of 92.0 g/mole. What is the molecular
formula of this substance?
33Empirical Formula from Composition
- A substance has the following composition by
mass 60.80 Na 28.60 B 10.60 H -
- What is the empirical formula of the substance?
- Consider a sample size of 100 grams
-
- This will contain 28.60 grams of B and 10.60
grams H -
- Determine the number of moles of each element
-
- Determine the simplest whole number ratio of each
element -
34Determination of Empirical Formulas using
combustion analysis data for organic compounds
- Experimental method that uses the mass of
starting materials and masses of water and carbon
dioxide produced to solve for the emp. Formula of
organic compounds. - Steps?
35Predicting Quantities of Products Based on
Quantities of Reactants Use(use concept/road
map)
36How do we do this?
- Predicting Quantities of Products Based on
Quantities of Reactants - Start from a balanced equation
- Use concept/road map
- Use dimensional analysis with (a) molar mass/ GFM
and (b) mole ratios as the basis of conversion
factors
37Practice Problem (Practice ex. P. 103).
- The decomposition of potassium chlorate is
commonly used to prepare small amounts of oxygen
gas in the laboratory. How many grams of oxygen
gas can be prepared from 4.50 g of potassium
chlorate?
38Limiting reagents(reactants) problems(Start with
POGIL Limiting reactants)
- Start with the balanced chemical equation
- Determine moles of reactants
- Setup tables (initial, change and end (final)
or ICE charts - Identify the limiting reagent/reactant
- Finish the problem using dimensional analysis
39(No Transcript)
40 Activities and Problem set X
- Ch 3 Problems TO DO write out questions and
answers show work - all GIST, sample practice exercises,
Visualizing concepts, - end of chapter 3 exercises 10, 11 (b,e,g), 12
(d,g), 14, 15, 17, 19, 23 (b,d), 26d, 27, 29, 33,
35, 37, 41, 43, 47, 53, 59, 63, 67, 68, 71, 73,
75, 80, 105
- TB ch. 3 all sections required for regents, SAT
II and AP exams - POGIL activities on chemical reaction equations,
limiting reactants, etc - Lab activities
- Determination CuxOy formula
- Percent composition of water in a hydrate
- Others - TBD
- Road/Concept map (provided)
- Online practice quiz due by ______