CHEM 060 Practice Final Exam
This 2-hour exam has three parts and 14 problems in total. Please make sure you answer all
questions and show work if applicable. If a problem requires any unit conversions or constants,
they will be given in that problem. To find any molar masses, a periodic table is included
separately. You may use no other materials except for a scientific calculator and blank scratch
Multiple Choice Questions (20 points, 4 each). Circle ONE answer.
1. Among the colors of visible light, blue light has the highest energy per photon. Red light
has the lowest energy and yellow is in between. What can you conclude about which
color of light has the longest wavelength?
A) Red light
B) Yellow light
C) Blue light
D) No conclusion can be drawn from the given information
2. Rank the following elements by atomic size, starting with the largest atom: Gallium,
Rubidium, Fluorine, Sulfur
3. A diver who believes that Heliox is a scam is planning to go on a very deep dive (beyond
70 m depth) and use regular air in his tank. What could happen?
A) Oxygen toxicity
B) Nitrogen narcosis
C) Both of the above
D) This is perfectly safe
4. Which of the following is NOT considered an intermolecular force?
C) London Dispersion
D) Hydrogen bonding
5. You are in charge of a volcanic lake that is saturated with carbon dioxide. More gas is
coming from underneath the lake and you are asked to prevent the carbon dioxide from
escaping above the lake, like in the disaster in Cameroon. Pipes are not an option in this
case. Which of the following would be a sound strategy?
A) Increase the temperature of the water
B) Reduce the pressure by removing water
C) Increase the pressure by adding pure water
D) Add salt to the water
Short Response Problems (30 points, 5 each). Show your work.
6. Write down the specified electron configurations for the following elements/ions:
a) N3- (regular configuration)
b) Si (electron orbital diagram)
c) Br (noble gas core notation)
7. You ascend a mountain and start to feel dizzy once the partial pressure of oxygen drops
to 0.10 atm. If the air at this altitude contains 21% oxygen by moles, what is the total air
8. If you dilute 50.0 mL of a 7.0 M CaCl2 stock solution to a volume of 2.00 L, what will be
the molarity of the resulting solution?
9. A sample of gas weighs 8.27 g and occupies a volume of 2.70 L at 88°C and 975 mmHg.
What is the molar mass of the gas? Given: 1 atm=760 mmHg. R=0.0821 L*atm/mol*K
Bonus: What gas do you think this is?
10. The heat of fusion of ice is 6.01 kJ/mol. How much heat is extracted from a glass of
water if you add 5 ice cubes weighing 6 grams each? Bonus (requires effort): what is the
final temperature if you started with 170 grams of water at 20°C?
11. Following an incident of road rage on the way to your exam, you eat 999 grams of sugar
candy to prevent your blood from boiling. By how much does the boiling point of your
blood increase if you have 5.00 kg of blood in your body? Assume your blood is pure
water and the candy is pure glucose with a molar mass of 180.2 g/mol. The boiling point
elevation constant for water is Kb=0.512°C/m where m is the regular unit for molality.
Long/Multi-part Problems (50 points total). Show your work where applicable.
12. Sulfuric acid can dissolve aluminum metal according to the following reaction.
2 Al(s)+3 H2SO4(aq)→Al2(SO4)3(aq)+3 H2(g)
Suppose you wanted to dissolve an aluminum block with a mass of 29.0 g and you have
1.80 L of 1.00 M sulfuric acid available.
Determine the limiting reactant. What is the theoretical yield of aluminum sulfate?
After the reaction is complete, you weigh the aluminum sulfate and it has a mass of
145 g. What is the percent yield of aluminum sulfate?
13. For each of the following compounds, complete the following steps:
1. Determine whether the compound is molecular or ionic.
2. Draw the Lewis structure for the compound, including lone pairs.
3. Determine the molecular geometry if the compound is molecular. If the compound is
ionic, determine the geometry of the anion (negative ion).
4. What is the dominant intermolecular/inter-particle force for this compound?
Given: Electronegativity of H: 2.1, Cl: 3.0, C: 2.5, F: 4.0, N: 3.0
Bonus: Rank the above compounds by their boiling points, starting with the highest.
14. Ammonia can be synthesized by this reaction:
3H2(g) +N2(g) → 2NH3(g)
a) Assume the reaction occurs at STP (1 atm, 273 K). How many liters of ammonia can
theoretically be produced if 202 g of hydrogen react completely?
Given: R=0.0821 L*atm/mol*K
b) The reaction enthalpy for the above reaction is -92.4 kJ/mol. Is heat released or consumed
in this process, and how much?
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