Honors Chemistry
Midterm Review Problem Stations
Introduction:
Each lab station has a set of questions/problems for you to solve in your group.
The answers to each station should be written on a separate sheet of paper and you must
use a different recorder for each station. In groups of 4 or 5 one or two people will serve
as the recorder twice.
At the end of the lab period staple all 6 answer sheets together IN ORDER and
write the names of all group members on the station 1 answer sheet. The grade will be
determined based on both accuracy and effort.
Station #1
(Unit 1 – Dimensional Analysis & ‘The Lab”)
1. If you have 12.47 g of mercury, how many cups of mercury do you have? The density of mercury
is 13.6 g/mL. See the equations & constants section of your reference book for other conversions.
2. A flooring company is going to replace the tiles on the floor of an office building and each tile is
12 inches by 12 inches. If the building contains 22 rooms and each room measures 12.0 meters by
15.0 meters, how many floor tiles will they need? (assuming no waste resulting from the need to
cut tiles, calculate the exact number of tiles based on the measurements)
3. Identify the following pieces of lab equipment by name:
4. When working in the lab a student found the density of an object to be 2.99 g/mL. If the actual
density of the object is 2.65 g/mL, which of the following are possible reasons for the outcome?
A.
B.
C.
D.
The measured mass was larger than actual
The measured volume was larger than actual
Both the measured mass and volume were larger than actual
Both the measured mass and volume were smaller than actual
Station #2
(Unit 2 –Nomenclature)
Name the following ionic compounds.
Write the formulas for the following ionic compounds.
1. AlCl3 ______________________________
1. Aluminum Phosphate _______________________
2. MnClO4 __________________________
2. Iron (II) Oxide _____________________________
3. Fe2O3 _____________________________
3. Potassium Nitride __________________________
4. TiNO3 ____________________________
4. Silver Nitrate ______________________________
5. KNO3______________________________
5. Nickel (II) Chloride _________________________
Name the following covalent compounds.
Write formulas for the following covalent compounds.
1. P4S5 ________________________________
1. tetrasulfur heptahydride ___________________
2. SO2 ________________________________
2. diphosphorous trisulfide ____________________
3. SeF6 ________________________________
3. trinitrogen pentaoxide_____________________
4. Si2Br6 _______________________________
4. silicon tribromide __________________________
5. SCl4 ________________________________
5. diboron tetrabromide _______________________
Mixed Ionic & Covalent: Write the formula or give the appropriate name for each compound given below.
1. KNO3 ________________________________
7. Manganese (IV) Sulfide ______________________
2. NF3 _________________________________
8. Si4Br9____________________________________
3. Rubidium Sulfate ______________________
9. Calcium Chloride __________________________
4. B2Si _________________________________
10. MgCl2 __________________________________
5. carbon tetraiodide _____________________
11. Cr2S ____________________________________
6. triphosphorous pentachloride ____________
12. Vanadium (V) Bromide ____________________
Station #3
(Unit 3 – Stoichiometry: Part I
Empirical & Molecular Formula)
1. Nickel reacts with sulfur to form a sulfide. If 2.986 g of nickel reacts with
enough sulfur to form 5.433 g of the compound, what is the empirical formula of
the compound? What is the correct chemical name for this compound?
Empirical Formula:
Name of Compound:
2. How many grams are there in a sample of 2.88x1035 molecules of C6H12O6?
3. What are the percentages of each of the elements in the compound Al2(SO4)3?
Station #4
(Unit 3 – Stoichiometry)
1. A factory that builds cars is doing a check of its inventory in order to determine if it needs to
order more parts from its suppliers in order to meet demand for its new model. In order to make
each car, they need 2 seats, 1 steering wheel, 4 brake rotors, 5 tires (don’t forget the spare!), and
1 windshield. We can think of the finished car as a product, and each of the materials needed to
make it as the reactants of a chemical reactions. Based on this we can write the following
balanced CARmical (lol) equation that represents the manufacturing of a car:
2 seats + 1 steering wheel + 4 brake rotors + 5 tires + 1 windshield  1 car
Based on this equation, and the following info from their inventory check, use stoichiometry to
determine how many complete cars can be made and which auto part would be our most
limiting reagent (which part would we run out of first?). Be sure to show your work.
Part
Quantity in warehouse
Seat
Steering Wheel
Brake Rotor
Tire
Windshield
38
16
80
75
18
CONTINUE TO PAGE 2 OF STATION #4!!   
Station #4 (cont.)
(Unit 3 – Stoichiometry)
2. Manned space flight poses many challenges. Due to the remote nature and the difficulty getting
to and from the International Space Station (ISS) many logistical hurdles must be crossed.
Everything from obtaining food and water, to what to do with the waste produced becomes a
daunting task that must thoroughly be thought out way ahead of time. One of the major
challenges on board the ISS is what to do with the carbon dioxide exhaled from the crew of the
station. One of the ways that NASA and ESA handle this is by installing scrubbers that remove
carbon dioxide from the air that is circulated within the ISS. These scrubbers are able to do this
because they are filled with a compound called lithium hydroxide. Lithium hydroxide reacts with
carbon dioxide to form water and lithium carbonate via the following unbalanced chemical
reaction.
_____ LiOH(s) + _____ CO2(g)  _____ Li2CO3(s) + _____ H2O(g)
The scrubbers on the ISS contain 6.00 kg of LiOH pellets. Based on this information, determine
the number of kg of CO2 that each scrubber can remove from the cabin of the ISS.
Assuming that these scrubbers provided all of the CO2 removal (they don’t) and assuming that
the average astronaut produces 34.1 moles of waste CO2/day and the ISS is staffed by three
astronauts, how long would one scrubber last before it had to be changed out with a new one?
Station #5
(Unit 4 – Reactions in Aqueous Solutions)
1. What is the molarity of a solution prepared by adding 15.50 g of potassium
chromate to water if the total volume of the solution is brought to 2550 mL?
2. How many grams of potassium hydroxide are required to prepare a 550 mL
solution of 1.4 M KOH?
3. Given the reactants below, first write a balanced chemical equation for the
reaction that will occur. Identify any compounds that would be precipitates with
the appropriate symbol in parenthesis after the formula.
Copper (II) acetate + sodium hydroxide 
4. Silver nitrate reacts with ammonium chloride in a given chemical reaction.
a. Write the complete balanced chemical reaction.
b. Write the net ionic equation.
c. Identify any precipitates.
d. Identify any spectator ions.
Station #6
(Unit 4 – Acids/Bases &
Unit 5 – Thermodynamics)
1. Write the dissociation equation for the strong acids or bases below:
a. Sr(OH)2 (aq) 
b. HNO3 (aq) 
2. According to the Brønsted-Lowry theory of acids/bases, predict the products of
the reaction and thenidentify each substance in the equation below as an acid,
base, conjugate acid, or conjugate base:
H2SO4
+
H2O
↔
3. What are the pH, pOH, [OH-], and [H+] of a solution with an H2SO4 concentration
of 2.34 x 10-4 M? Is this solution acidic or basic?
pH =
pOH =
[H+] =
[OH-] =
4. A 15.75 g piece of iron absorbs 1086.75 J of heat energy and the temperature
changes from 25°C to 175°C. Calculate the specific heat capacity of iron.
5. How many grams of water can be heated from 20.0°C to 75.0°C using 12.5 kJ?