Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Date
In Class
Homework
10/22 Thur
Counting By Mass Lab
10/23 Fri (mole day!!!)
THE MOLE! in room 137
10/26 Mon (LSM)
More on the Mole
Watch empirical and molecular
formula video.
10/27 Tue
% Composition & Calculating
Empirical Formulas
work on problems in the packet
(1-7 on page 8)
10/28 Wed.
Nomenclature Review
Prelab for Hydrated Crystal Lab
10/29 Thurs
Hydrated Crystal Lab
10/30 Fri
NO SCHOOL! whoo hoo!!!
work on problems in the packet
(8- 20 on pages 9)
11/2 Mon
Work on Unit Packet
Finish all problems in Unit Packet
(21 – 28 on page 10-11)
11/3 Tues
Review for Chapter 10 Test
Study for Test
11/4 Wed
Chapter 10 Test
prelab for Types of Chemical
Reactions
11/5 Thur
Types of Chemical Reactions
1
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Notes for chapter 10:
1. What is a mole?
2. What units can a mole be converted to/from:
a.
b.
c.
MOLE/PARTICLE (MOLECULES AND ATOMS)
3. How many molecules are in a mole?
4. When converting from molecules/atoms you _____________________________________
5. When converting from moles to molecules/atoms you ______________________________
Mole/Particle Practice:
26
a. How many moles are in 5.3 x 10 atoms of copper?
b. How many molecules are there in 3.5 moles of sucrose?
2
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
MOLE/MASS (GRAMS)
6. Define atomic mass in terms of moles:
a. What is the atomic mass of 1 mole of a hydrogen atom?
b. What is the atomic mass of 1 mole of an aluminum atom?
7. Define molar mass.
8. Show how you calculate the molar mass of water (H2O)
9. When converting from grams to moles you _____________________________________
10. When converting from moles to grams you _____________________________________
Mole/Gram Practice:
a. How many grams of Iron are in 2.7 moles of Iron?
b. How many moles of Zinc are in 15 grams of Zinc?
c. How many grams are in 23 moles of CO2?
d. How many moles are in 562 grams of CO2?
e. Calculate the molar mass of ammonium carbonate
f.
How many grams are in3.5 moles of ammonium carbonate?
3
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
MOLE/VOLUME (LITERS)
11. What does STP stand for?
12. What is the temperature and pressure at STP?
13. At STP when converting from liters to moles you _____________________________________
14. At STP when converting from moles to liters you _____________________________________
Mole/Liter Practice:
a. How many liters are present in 10 moles of H2 at STP?
b. How many moles are in 17 L of water vapor?
THE MOLE: A BRIGE BETWEEN PARTICLES, GRAMS, AND LITERS
15. List the steps used in calculating how many molecules of H2O are present in 10.8 grams?
16. How many liters are present in 6 grams of O2 gas at STP
4
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Video on Empirical and Molecular Formulas: Link: https://www.youtube.com/watch?v=wnRaBWvhYKY or
search Tyler Dewitt Empirical and Molecular Formulas
Video title is: Empirical Formula and Molecular Formula Introduction
Guided Notes
What is a molecular formula?
Questions
What is an empirical formula?
Use ethene (which is really butene….) as an example of a molecular and empirical
formula.
Write the molecular formula and empirical formula for cyanuric triazide
What do you divide by to get the empirical formula for C5H10O5?
What is the empirical formula for C5H10O5?
When is the molecular formula the same as the empirical formula?
Why can many compounds have the same empirical formula? Show an example of
several molecular formulas that come from the same empirical formula.
Check your learning Practice.
Write the empirical formulas for the following compounds:
1. H2O2
2. H2O
3. C2H10O4
4. C5H10O2
Answers to above 1. HO
2. H2O
3. CH5O2
4. C5H10O2
5
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Percent Composition and Calculating Empirical Formulas:
1. What is a percent composition?
2. Write the equation for calculating % composition? % composition =
x100
3. Using the molar mass we calculated for ammonium carbonate from page 3 e, show how to calculate the
percent of each element in the compound.
a. N
b. H
c. C
d. O
4. Calculate the percentage composition for all the elements in barium nitrate?
5. Write each step for how to calculate the empirical formula of a compound using mass or percent composition.
a. Step 1.
b. Step 2.
c. Step 3.
d. Step 4.
6
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
6. Use the steps in 5. to calculate the empirical formula of a compound that contains 28.4 g copper and 71.6 g
bromine?
7. Follow the steps in 5. to calculate the empirical formula of a compound that contains 36.4% Carbon and
63.6% Nitrogen
7
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Homework Practice Problems – answers on last pages
1. Find the molar mass (g/mole) of:
a. Na
e. MgI2
b. C
f. AgClO2
c. O2
g. Cu(NO3)2
d. KOH
h. Mg3(PO4)2
2. Calculate the mass (grams) of:
a. 1.00 mole of CaCl2
b. 2.0 mol of Al
c. 0.50 mol H2SO4
d. 0.10 mole of Na2O
3. Calculate moles in:
a. 16.0 g of O2.
b. 3.2 g of H2O
c. 168 g of NaHCO3
d. 6.25g Al2O3
4. Calculate the number of molecules in:
a. 3.0 moles OF ANYTHING
b. 32 mol of CH4
c. 1.4 mol of NH3
d. 2.5 mol O2
5. Calculate the number of moles in:
a. 1.204 x 1024 molecules
b. 3.5 x 1024 molecules of HCl
c. 6.5 x 1029 molecules of H2SO4
d. 3.5 x 1012 molecules of SO3
6. Calculate the number of moles in:
a. 45 L F2
b. 3.5 L SO2
c. 78.9 L CO
7. Calculate the volume in liters of:
a. 4.50 mol NO2
b. 8.5 mol CO2
c. 105 mol CO
8
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
8. Determine mass in grams of 40.0 moles of sodium carbonate.
9. How many grams are in 0.020 moles of Sn
10. How many liters are in 6.0 mol O2
11. Calculate moles in 510.0 g of aluminum sulfate.
12. How many moles are in 40.0 g Na2CO3
13. How many moles are in 3.00 L of N2
Moles are the Bridge between units:
14. Determine the mass in grams of 2.35 molecules of C12H22O11
15. How many liters are present in 100g of CO2 (at STP)?
16. How many sulfur atoms are present in 25.0 grams of H SO4?
2
17. How many atoms are in 2.00 grams of carbon? (2 steps)
18. Determine the mass of 50L of CO.
19.(challenge) How many moles of carbon atoms are in 3.00 grams of C2H5OH?
Percent Composition:
20. Determine the percentage composition of each element in the following compounds:
a. magnesium iodide, MgI2
%Mg = _________
% I = _________
b. calcium chlorate, Ca(ClO3)2
% O = ______
%Ca= _______
%Cl = _______
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Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Empirical vs. Molecular formulas
21. Write the empirical formula for each of the following compounds. (Not all will need to be changed!)
a. Na2O2
____________________
d. Cu2C2O4
____________________
b. Li2SO4 ____________________
e. CaC4H4O6
____________________
c. Hg2F2
f. C6H6
____________________
____________________
Calculating Empirical Formulas
22. What is the empirical formula of a compound that contains 1.67 g of Ce and 4.54 g of I?
23. What is the empirical formula of benzoic acid (a food preservative) if it contains 68.8% carbon, 4.95% H, and 26.2% O
by mass?
24. Calculate the empirical formula for a compound made up of 63.6% iron and 36.4% sulfur.
25. Calculate the empirical formula of a hydrate that is 48.8% magnesium sulfate and 51.2% water (from lab)
26. Calculate the formula for a hydrate that is 37.07% sodium carbonate and 62.93% water (from lab)
10
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
Nomenclature Practice:
27. Provide the name for each of the following:
a. PbCl2
g. H2CO3
b. Hg(NO3)2
h. Sn3(PO4)2
c. AgF
i. N3Br7
d. Ca(OH)2
j. H2SO3
e. HF
k. HNO3
f. S4O6
l. Cu(C2H3O2)2
28. Provide the formula for each of the following:
a. Iron (III) oxide
g. acetic acid
b. aluminum iodide
h. carbon monosulfide
c. Lead (II) sulfate
i. phosphoric acid
d. mercury (II) nitrate
j. chlorous acid
e. tin (IV) hydroxide
k. hydroselenic acid
f. ammonium sulfide
l. disulfur noniodide
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Unit 6. Chapter 10: The MOLE!
Chemistry – Chap. 10 HW- Answers
1.
a. 22.99 g
b. 12.01 g
e. 278.11 g
f. 175.32 g
Name:____________________________________
c. 32.00 g
g. 187.56 g
d. 56.11 g
h. 262.87 g
d. 6.2 g
2.
a. 110.98 g
b. 53.96 g
c. 49 g
3.
a. .500 mol
b. .18 mol
c. 2.00 mol
4.
a. 1.8 x 1024 molecules b. 1.9 x 1025 molecules
d. 1.5 x 1024 molecules
c. 8.4 x 1023 molecules
5.
a. 2.000 mol
b. 5.8 mol
c. 1.1 x 106 mol
6.
a. 2.0 mol
b. .17 mol
c. 3.52 mol
7.
a. 101 L
b. 190 L
c. 2350 L
8.
40.0 moles Na2CO3 x 106g/1mol = 4240g
9.
2.4 g
d. .0613 mol
d. 5.8 x 10-12 mol
10. 134 L
11. 510.0 g aluminum sulfate x 1molH2SO4/342g = 1.5 mol
12. 0.377 mol
13. 0.139 mol
14. 2.35 molecules C12H22O11  6.02 x 1023 molecules x 342g/mol = 1.34 x 10-21 g
15. 100g CO2  44g x 22.4L/mol = 50.9 L
16. 1.5 x 1023 atoms S
17. 2.00 grams C  12 gC x 6.02 x 1023 atoms/mol = 1.0 x 1023 atoms C
18. 50L of CO  22.4L x 28g/mol = 62.5 g CO
19. 3.00 grams C2H5OH  46g x 2C/1 C2H5OH = 0.13 mol C atoms
20. a. %Mg= 24.3 / 278.3 x 100 = 8.7%
b. Cl = 71/207 x 100 = 34.3%
%I = 254/278.3 x 100 = 91.3%
O = 96 / 207 x 100 =46.4%
21. Write the empirical formula for each of the following compounds. (Not all will need to be changed!)
a. Na2O2 _NaO_______________
d. Cu2C2O4 ___CuCO2
b. Li2SO4 _ Li2SO4
e. CaC4H4O6 __ CaC4H4O6
c. Hg2F2 __HgF
f. C6H6 ___CH
12
Unit 6. Chapter 10: The MOLE!
Name:____________________________________
22. What is the empirical formula of a compound that contains 1.67 g of Ce and 4.54 g of I?
1.67g/140= 0.012mol
0.012/0.012 = 1
4.54g/127 = 0.036 mol
0.036/0.012 = 3
CeF3
23. What is the empirical formula of benzoic acid (a food preservative) if it contains 68.8% carbon,
4.95% H, and 26.2% O by mass?
68.8g C/12 = 5.73 mol C
5.73/1.64 = 3.5
x2
7.0
4.95g H/1 = 4.95 mol H
4.95/1.64 = 3
x2
6
26.2 g O / 16 = 1.64 mol O
1.64/1.64 = 1
x2
2
C7H6O2
24. Calculate the empirical formula for a compound made up of 63.6% iron and 36.4% sulfur.
63.6/55.8 = 1.14
FeS
36.4g/32 = 1.14
25. Calculate the empirical formula of a hydrate that is 48.8% magnesium sulfate and 51.2% water
48.8g/120 = 0.405 mol MgSO4
0.405/0.405 = 1
51.2 g/18 = 2.84 mol H2O
2.84/0.045 = 7
MgSO4 7 H2O
26. Calculate the formula for a hydrate that is 37.07% sodium carbonate and 62.93% water
37.07g/106 = 0.356 mole (Na)2CO3
0.356/0.356
1
62.9g / 18 = 3.49 mol H2O
3.49 / 0.356
9.8
Na2CO3 * 10 H2O
27. Provide the name for each of the following:
a. Lead (II) chloride
b. mercury (II) oxide
d. calcium hydroxide
e. hydrofluoric acid
g. carbonic acid
h. tin(II) phosphate
j. sulfurous acid
k. nitric acid
c. silver fluoride
f. tetrasulfur hexoxide
i. trinitrogen heptabromide
l. copper (II) acetate
28. Provide the formula for each of the following:
a. Fe2O3
g. HC2H3O2
b. Al I3
h. CS
c. PbSO4
d. Hg(NO3)2
e. Sn(OH)4
f. (NH4)2S
i. H3PO4
j. HClO2
k. H2Se
l. S2I9
13