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Chemistry (Spring) Final Exam Topics and Practice
The final will be completely multiple-choice Scan-tron. There will be about 100 questions. You will have two
hours to complete the test, but I do not think that it will take everyone the entire class. The topics to be covered
on the test are listed below. You will be given a periodic table and all other tables for the final, BUT you need
to bring a calculator.
 You may use a HANDWRITTEN 8.5” x 11” piece of paper (FRONT ONLY)
 Study from your notes, old tests and quizzes, homework, your comp book, and the book
 On test day, please bring:
o #2 pencils and erasers (test will be scan-tron)
o Scrap paper to do your work
o CALCULATOR
o YOUR BOOK!
o Something to do after taking the final
What do I need to get on the final?
My Current grade (%) = ____________
Overall Grade I Want – Be realistic!! (%) = ____________
1. My Current grade × 0.80 = X
2. Overall Grade I Want – X = Y
3. (Y ÷ 20) 100= percent I have to get on the final in order to get the overall grade I want
Gases
 Know gas properties (pressure, temperature, volume, number of moles)
 Boyle’s Law, Gay-Lussac’s Law, Charles’ Law, Combined Gas Law, Ideal Gas Law
 Calculate pressure, temperature, volume and number of moles as appropriate
 Law of Partial Pressure (and how it relates to water pressure)
 Gas Stoichiometry
Acid/Base/Equilibrium
 Properties of acids and bases, definition of indicators
 Arrhenius and Bronsted-Lowry definitions of acids and bases
 Calculating pH, pOH, [H+], and [OH-] of acids and bases
 Neutralization Reactions and Titrations
 Reversible Reactions/Equilibrium: Weak acids and bases
Thermochemistry
 Understand parts of a heating curve – terms for change in state (melting, etc.)
 Specific Heat (the concept, as well as calculations using specific heat), Heat of Fusion and Heat of
Vaporization
 Perform multi-step calculations using specific heat, heat of fusion and heat of vaporization
 Definition of endothermic, exothermic, enthalpy, and entropy
 Calculate enthalpy, entropy and Gibb’s Free Energy (using the chart)
 Determine whether a reaction is spontaneous or non-spontaneous (using Gibb’s Free Energy)
Solutions
 Express and calculate concentrations of solutions in molarity
 Explain freezing point depression and boiling point elevation in terms of particles
Organic
 Name and Draw organic molecules
 Know how to name and draw the functional groups
 Addition and Dehydration reactions
 Polymers
Nuclear
 Nuclear Reactions
 Fission vs. Fusion
PRACTICE!
1. Which of the following is NOT a property of gases?
a. Gases are compressible
b. Gases can expand
c. Gases can spontaneously diffuse
d. Gases are very dense
e. Gases have high fluidity
2. When 45.3 grams of C3H8 reacts with oxygen gas, how many liters of CO2 are produced if the reaction is carried
out at 56°C and a pressure of 780 mmHg? A. 3.1 B. 81
C. 61
D. 0.11
3. If volume and number of moles are constant, the pressure of a gas varies
a. Directly
b. Inversely c. No relationship exist
with temperature.
4. What is the volume of one mole of gas at STP?
a. 1 liter
b. 12 liters
c. 22.4 liters
d. It depends on the gas since all gases have different densities
5. Which of the following is NOT true at STP conditions?
a. Temperature is at 0°C and pressure is at 1 atm
b. Temperature is at 273 K and pressure is at 760 mmHg
c. The volume of 1 mol of He gas is 22.4 L
d. The volume of 1 mol of Cl2 gas is 12 L
e. All of the above are true
6. You have a 2.4 L container of air at 273 K and 1 atm. From out of nowhere, Bigfoot stomps on it, decreasing the
container’s volume down to 0.5 L and increasing the pressure to 8 atm. How hot is the air in the container now?
a. 0.035 K
b. 28 K c. 455K d. 600 K e. None of the above
7. Which of the following has the most molecules?
a. 2.00 L of CH4 at 0oC and 2.00 atm
b. 2.00 L of N2 at 0oC and 1.00 atm
c. 2.00 L of O2 at 20oC and 1.00 atm
d. 2.00 L of CO2 at 50oC and 1.25 atm
e. 2.00 L of CO at 0oC and 1.25 atm
8. In an experiment, 5 gram samples of Ag, Cu, Au and Al were all heated to 100°C and were then allowed to
simultaneously cool for 30 seconds before their temperatures were measured. Which metal will have the lowest
temperature?
a. Ag (specific heat = 0.233)
b. Cu (specific heat = 0.385)
c. Au (specific heat = 0.129)
d. Al (specific heat = 0.895)
e. Can’t tell from the information that is given
9. Which of the following will have the greatest specific heat?
a. Glass b. Steel c. Styrofoam
10. It takes 31.2 joules of heat to change the temperature of a sample of silver by 12°C. What is the mass of this
silver? (specific heat of silver = 0.233 J/g°C)
a. 0.090 grams
b. 0.607 grams
c. 11.2 grams d. 1600 grams e.None of the above
11. A piece of metal is sitting in boiling water. You transfer the metal to a cup of cold water and assume that no heat
is lost to the environment. Use the following data to determine the specific heat capacity of the metal.
Mass of cup
2.0 g
Mass of cup and water
102.0 g
Initial temp. of water
22 oC
Final temp. of water
26 oC
Mass of metal
12.0 g
Temp. of boiling water
100.0 oC
o
a. 16.7 J/g C
b. 9.07 J/goC
c. 1.88 J/goC
d. 0.717 J/goC
12. Ice Melting at room temperature is …
a. An endothermic and spontaneous process
b. An exothermic and spontaneous process
c. An endothermic and non-spontaneous process
d. An exothermic and non-spontaneous process
e. None of the above
13. What is enthalpy?
a. A measure of heat or energy
b. A measure of randomness and disorder
c. A measure of how spontaneous a reaction will be
d. A measure of the number of cows that can jump over the moon
e. None of the above
14. When the ∆H of a reaction is negative:
a. The reaction is spontaneous
c. The reaction is non-spontaneous
b. The reaction is exothermic
d. The reaction is endothermic
15. Calculate the change in enthalpy for 2H2O(g)
a. 35.6 kJ
b. 268.2 kJ
 2H2 + O2
c. 1343.3 kJ
d. 483.6 kJ
16. Which of the following is not a characteristic of a base?
a. slippery
b. changes indicators colors
c. conducts electricity
d. proton donor
17. 79 ml of KOH is added to 23 ml of 0.305 M H2SO4 to neutralize it. What is the molarity of the base?
a. 1.3M
b. 0.007M
c. 0.014M
d. 0.177M
e. 13.9 M
18. What is the pH of the base from #15?
A. 0.752
19. If the pH of a solution is 7, it is _________ .
20. If HCl is 0.000356 M, what is the pOH?
a. 3.4
b. 10.6
B. 1.85
a. an acid
C. 13.24
b. a base
c. 3.1
c. both
D. 8.9
d.neither
d. 10.9
21. If you dissolve 5 g of C12H22011 in 0.5 L, what is the concentration?
a. 10 M
b. 0.2 M
c. 0.03 M
22. What doesn’t completely ionize in an aqueous solution?
a. Conjugate acid
b. Strong acid
c. Weak acid
23. What do you call 2 substances that are related to each other by the donating and accepting of a single proton?
a. Conjugate acid-base pair
b.Weak bases
c. Strong acids
d.Strong bases
24. In the reaction NH3+ H2O <--> NH4+ + OH-, the two Bronsted-Lowry acids are…
a. NH3 and OHb. NH4+ and H2O
c. OH- and H2O
d. OH- and NH2-
25. How does a nuclear reactor generate energy?
a. boiling water b. cooling water
c. bringing water to a simmer
d. freezing water
26. If a tennis ball undergoes a fission reaction, what would the ball be doing?
a. bouncing up and down
b. sitting still
c. splitting in half
d. coming together with another ball to make a big tennis ball
27. What kind of reaction happens in a nuclear power plant
a. fusion
b. fission
c. thermonuclear
d. alphanumeric
28. What would this molecule be called?
a. 2-methylpentanol
b. 4-methylhexanoic acid
c. 2-methylpentanoic acid
d. heptanoic acid
29. How many carbons are in 3,3,5,5-tetramethyl-2-hexanol?
a. 6
b. 14 c. 10 d. 8
30. Butyl pentanoate is a(n) _____________.
a. carboxylic acid
b. ether
c. ester
31. The previous problem has a formula of …
a. C5H10O
b. C9H18O
c. C9H18O2
d. ketone
d. C4H9O2
32. 2-ethoxypentane is a(n) _____________.
a. carboxylic acid
b. ether
c. ester
33. The previous problem has a formula of …
a. C7H10O
b. C7H16O
c. C7H18O2
Answers:
1D
2B
16D
17D
31C
32B
3A
18C
33B
4C
19D
5D
20B
6C
21C
7A
22C
d. ketone
d. C5H9O2
8C
23A
9C
24B
10C
25A
11C
26C
12A
27B
13A
28C
14B
29C
15D
30C