1
11/18
2
3
4
5
6
7
8
9
10
11
Tent.
12/6
Classwork
Introduction to the Mole Activity
(40 Points)
Mole & Mole-Bile presentations
Notes: Molar Mass
Daily Quiz
1-Step Molar Conversions
Mole Conversions Lab
Daily Quiz
2-Step Molar Conversions
Daily Quiz
Percent Composition
Daily Quiz
Empirical Formulas
Percent Composition Lab (20 Points)
Daily Quiz
Molecular Formulas
Finish Daily Quiz (25 Points)
Homework & Extra Credit Due (50 Points)
Formal Lab—Determining an Empirical Formula
(50 Points)
Go over homework, daily quiz and any lab questions.
Chapter 10 Test (100 Points)
Homework Grades:
A(50/50)
B (45/50)
C (40/50)
D (35/50)
E (33/50)
F (30/50)
0/50
6/6 Homeworks Complete
5.5/6 Homeworks Complete
5/6 Homeworks Complete
4.5/6 Homeworks Complete
4/6 Homeworks Complete
3/6 Homeworks Complete
Less Than 3/6 Homeworks Complete
Homework
Define & Study Chapter 10 Key Terms
HW1: Worksheet A
HW2: Worksheet B
Finish today’s lab
HW3: Worksheet C
HW4: Worksheet D
HW5: Worksheet E
Complete Lab for Homework
HW6: Worksheet F
Start Formal Lab Report
Study for Chapter 10 Test
Complete Lab Report
Extra Credit:
5 Points: Text p. 317 #91
3 Points: Text p. 319 #1-15
3 Points: Make a 0.5 mole aluminum foil sculpture
of a mole (the critter). The sculpture will be checked
and weighed for accuracy.
10 Points: Create a poster illustrating the following:
1) How a GC/MS works
2) How a GC/MS uses masses to verify the
identification of samples.
3) The applications of a GC/MS
Top Pair for Chapter 9:
Matt Marsh & Hong Lee
Total Possible Points This Chapter: 285 + 25 Possible Extra Credit Points
WORKSHEET A—MOLAR MASS
Find the molar mass for each of the following compounds.
1) H3PO4
14) zinc acetate
2) AlCl3
15) copper(I) sulfate
3) Dy(OH)3
16) carbon dioxide
4) K2C4H4O6
17) calcium bicarbonate
5) H2SO4
18) hydrofluoric acid
6) N2O5
19) aluminum nitrate
7) CuSO45H2O
20) ammonium sulfate
8) Sn(OH)4
21) iron(II) phosphate
9) (NH4)3PO4
22) magnesium nitride
10) Fe(C2H3O2)3
23) strontium hydroxide
11) SO2
24) sodium oxide
12) Pr(OH)3
25) oxygen difluoride
13) K4Fe(CN)6
26) barium chloride
WORKSHEET B
1-STEP MOLAR CONVERSIONS
1. A bottle of PbSO4 contains 158.1 g of the compound. How many moles of PbSO4 are in the bottle?
2. How many moles of magnesium bromide contain 5.38 x 1024 formula units?
3. A chemical reaction produces 0.37 mol N2 gas. What volume will that gas occupy at STP?
4. Find the mass of 1.112 mol of hydrofluoric acid.
5. How many moles of ethane (C2H6) contain 8.46 x 1024 molecules?
6. A tube with a volume of 3.68 L contains how many moles of neon gas at STP?
7. A 2.5 g sample of calcium nitrate was heated. How many moles of calcium nitrate were heated?
8. How many atoms are there in 1.638 x 10-9 mole of lithium?
9. If you use 30.6 g of methanol (CH3OH) to start a fire, how many moles of methanol did you use?
10. A container with a volume of 893 L contains how many moles of air at STP?
WORKSHEET C
MIXED CONVERSIONS
1. What is the mass of 0.438 mole of ammonium chloride?
2. How many formula units are there in 993.6 g of potassium sulfate?
3. How many grams are there in 15.5 x 1023 molecules of carbon dioxide?
4. What is the volume occupied by 4.20 moles of oxygen gas at STP?
5. How many moles are in 45.0 dm3 of methane gas (CH4) measured at STP?
6. A sample of carbon dioxide has a mass of 22.0 grams. What volume will the sample occupy
at STP?
7. A sample of N2 is composed of 3.01 x 1023 molecules. What is the mass of this sample?
8. A sample of methane (CH4) has a volume of 67.2 dm3 at STP. What is the mass of this
sample?
WORKSHEET D
PERCENT COMPOSITION
1. Find the percent composition of a compound that contains 2.7369 g of chlorine, 0.4116 g of
oxygen and 0.7971 g of phosphorus in a 3.9456 g sample of the compound.
2. What is the percent composition of SO2?
3. Determine if the following samples are the same compounds.
Sample A: 45.0 g sample containing 35.1 g Fe and 9.9 g O
Sample B: 215.0 g sample containing 167.7 g Fe and 47.3 g O
(Hint: Find the % composition of each and compare—Law of Definite
Proportions/Constant Composition)
4. Find the percent composition of a compound that contains 1.94 g of carbon, 0.48 g of
hydrogen and 2.58 g of sulfur in a 5.00 g sample of a compound.
5. A sample of an unknown compound with a mass of 0.847 g has the following composition:
50.51% fluorine and 49.49% iron. When this compound is decomposed into its elements, what
mass of each element would be recovered?
WORKSHEET E
EMPIRICAL FORMULAS
1. What is an empirical formula?
2. Which of the following formulas would be considered empirical formulas? There may be
more than one answer.
a) ribose (C5H10O5)
b) ethyl butyrate (C6H12O2)
c) chlorophyll (C55H72MgN4O5)
d) DEET (C12H17ON)
3. Which pair of molecules has the same empirical formula?
a) C2H4O2, C6H12O6
b) NaCrO4, Na2Cr2O7
4. Calculate the empirical formula for each of the following compounds:
a) 42.9% C and 57.1% O
b) a compound consisting of 0.40 mol Cu and 0.80 mol Br
c) 25.9% nitrogen and 74.1% oxygen
5. 1,6-diaminohexane is used to make nylon. What is the empirical formula of this compound if
its percent composition is 62.1% C, 13.8% H and 24.1% N?
WORKSHEET F
MOLECULAR FORMULAS
1. What is the difference between a molecular formula and an empirical formula?
2. Which has the largest mass?
a) three atoms of magnesium
b) one molecule of sucrose, C12H22O11
c) ten atoms of helium
3. What is the molecular formula for each of the following compounds?
a)
empirical formula: CH2
molar mass: 42 g/mol
b)
empirical formula: CH
molar mass: 78 g/mol
c)
empirical formula: CH2O
molar mass: 90 g/mol
4. Oleic acid is a component in olive oil. It is 76.5% C, 12.1% H and 11.3% O. The molar mass
of the compound is approximately 282 g/mol. What is the molecular formula of oleic acid?
5. Seratonin is a compound that conducts nerve impulses in the brain. Serotonin is 68.2% C,
6.86% H, 15.9% N and 9.08% O. The molar mass is 176 g/mol. What is the molecular formula
of serotonin?