Winter Break Problem Set(s) – Advanced Chemistry
Your midterm will be given on Monday, January 12th. This is before the actual midterm exams. This way
you will be able to spend the time slotted for our midterm doing test corrections, if necessary. The
following shows the breakdown of the midterm exam:
Topics Covered
Nomenclature
Empirical Formulas and Percent Composition
Balancing, Stoichiometry and Limiting Reagents
Redox
Significant Figures & Precision vs. Accuracy
Calibration Curves
Subatomic Particles
Possible Points
20
18
33
10
9
5
5
For your Winter Break work, there are 4 available problem sets. You must complete THREE of them –
your choice. I suggest picking whichever you need the most practice with. You can find all problem sets
posted online. If you do the 4th, you can earn extra credit and be extra prepared for the exam.
The worksheets don’t cover all topics, but we will spend two periods reviewing some more. The four
topics you can choose from are:




Nomenclature (quarter 1)
Empirical Formulas and Percent Composition (quarter 1)
Balancing and Stoichiometry (quarter 2)
Limiting Reagents (quarter 2)
All work should be done on lined sheets of paper.
Reminder…these must be your own work. Do not copy off of a peer (you will both earn a 0). If you do
not do this work, you will not be prepared for this exam. Put in the work!
Nomenclature Problem Set
Write formulas for the following compounds:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
sodium carbonite
nitrogen pentahydride
cobalt (IV) oxide
hexane
phosphorus acid
gallium persulfate
zinc (II) hyponitrate
hydronitric acid
ethanol
nonene
trioxygen tetrafluoride
carbonic acid
Write the names for the following compounds:
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
H3P
CS
Al(CN)3
HI
C4H10
HClO4
HC2H3O2
V2S4
C9H16
N2S2
Ti2(SO3)5
Write SIX of your own formulas and their corresponding names (#s 24-29).
Empirical Formulas and Percent Composition Problem
Set
1. Heptene
a. Write the formula
b. Write its empirical formula
c. Can an empirical formula and molecular formula ever be the same? Give an example.
d. Determine the percent composition of heptene (from part a). Show ALL work.
2. Titanium (II) hypocarbonate
a. Write the formula
b. Write its empirical formula
c. What is the difference between an empirical and molecular formula?
d. Determine the percent composition of each element in titanium (II) hypocarbonite.
Show ALL work.
3. A compound contains zinc, chlorine, and oxygen. It is 43.9% zinc and 23.6% chlorine.
a. What is the empirical formula of this compound? Show ALL work.
b. The molar mass of the compound is approximately 444 g/mol. Determine its
molecular formula. Show ALL work.
4. A compound is 27.3% potassium, 33.6% titanium, and 39.1% oxygen. Calculate its empirical
formula.
Balancing and Stoichiometry Problem Sets
Balance the reactions below and then answer the three stoichiometry problems that follow each
reaction.
Reaction 1:
___H2S + ___KOH  ___H2O + ___K2S
1. Balance the reaction.
2. How many grams of potassium sulfide are produced if you start with 22.3 grams of potassium
hydroxide?
3. You put 12.8 liters of 5.0 M sulfuric acid. How many molecules of water are produced?
Reaction 2:
___C12H26 + ___O2  ___CO2 + ___H2O
4. Balance the reaction.
5. How many moles of water are produced if you use 59.5 liters of oxygen gas?
6. If you put in 64.0 grams of C12H26, how many molecules of carbon dioxide are produced?
Reaction 3:
___C7H6O3 + ___O2  ___CO2 + ___H2O
7. Balance the reaction.
8. Assume that this reaction produces 565.5 kJ of energy. If you start with 5.3 liters of oxygen, how
much energy is produced?
9. How many moles of water are produced if you start with 12.8 grams of C7H6O3?
Limiting Reagents Problem Set
Use the reactions to answer the three questions that follow each one.
Reaction 1:
2Al + 3H2SO4  3H2 + Al2(SO4)3
You put 23.7 grams of aluminum and 7.6 liters of 4.0 M sulfuric acid into a reaction.
1.
2.
3.
4.
What is the limiting reagent?
What is the excess reactant?
How much excess remains after the reaction has finished?
How many molecules of aluminum sulfate are produced?
Reaction 2:
2BN + 3F2  2BF3 + N2
5.75 grams of BN and 6.37 grams of F2 are put into this reaction.
5. What is the limiting reagent?
6. How many grams of the excess is left over after the reaction is done?
7. How many moles of BF3 is produced?
Reaction 3:
C3H8 + 5O2  3CO2 + 4H2O
6.9 grams of propane and 34.9 liters of oxygen are put in the reaction.
8.
9.
10.
11.
What is the limiting reagent?
What is the excess reactant?
How many liters of carbon dioxide are produced?
What mass of water is produced?