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Module 13 Test
Test
is Closed Book & Closed Notes. 60 Minute Time Limit.
You are allowed to
use the Periodic Table on ALL tests. However, you are not allowed to use
the table that lists the names and their abbreviations.
Please use Table 13.1, 13.2, 13.3, and 13.4 in the Appendix of your
textbook for any of the questions on this test that you might
need a bond energy,
ΔHf , ΔS, ΔGf value. These are the only tables you
are allowed to use.
A.
True or False - Indicate which of the following are true (T) or false
(F): 1 point each
1. When solutes dissolve
exothermically, they release energy, which causes the solution to heat up.
2. From a chemistry point of
view, heat energy associated with a chemical reaction is considered potential
energy.
3. When a solution cools down
after the solute and solvent are mixed, the process is said to be endothermic,
which indicates that energy is being absorbed from the surroundings.
4. The units attached to ΔH are either kiloJoules (kJ)
or kilocalories (kcal).
5. A ΔH of 50 kJ/mole means that
50 kJ of energy change occurred from one mole of product consumed.
6. If the chemical reaction is
exothermic, the entire reaction will get hot.
7. A reaction coordinate of zero
means that the reaction has completed and all the products are formed.
8. The difference between the
vertical (y) position of the products and the vertical (y) position of the
reactants is the “ΔH” of the reaction.
9. If a chemical reaction is
exothermic, some of the potential energy stored in the reactants is converted
into kinetic energy.
10.
When calculating ΔS, the S of an element is not zero. All substances, even elements, have an
absolute entropy.
11.
The Gibbs Free Energy actually can tell one whether or not a reaction is
consistent with the Second Law of Thermodynamics.
12.
When a solute dissolves in a solvent, no chemical change occurred.
13.
The reaction, HCl + NaOH à H2O + NaCl + energy,
indicates an exothermic reaction.
14.
If a chemical reaction is endothermic, kinetic energy from the
surroundings is converted into potential energy stored in the products’
chemical bonds.
15.
The whole theory of evolution that is predicated on the belief that
simple life forms can evolve into complex life forms violates the Second Law of
Thermodynamics.
16.
According to the First Law of Thermodynamics, energy is never really
produced nor consumed by a chemical reaction.
It can only change forms.
17.
According to Dr. Wile, there are two types of energy: electric and gas.
For questions 18
through 20, please use the following diagrams.
Please answer with either a I, II, or III.
18. Diagram III shows an exothermic reaction.
19. Diagram II represents the reaction with the
lowest activation energy.
20. Diagram I has a ΔH of 300 kJ.
B.
Multiple Choice - Select the best possible answer for the
following: 1 point each
21. ΔH stands for which of the following?
a. the potential energy associated with a
substance.
b. the enthalpy of a molecule.
c. the potential energy change associated with a
reaction.
d. the heat involved in the reaction.
e. none of the involved.
22. What is the energy necessary to start a
chemical reaction?
a. ΔH
b. ΔHf
c. ΔS
d. Activation energy
e. None of the above
23. Which of the following is an acceptable unit
for entropy?
a. kJ / (g °C)
b. kJ / mole
c. kcals / (mole °C)
d. kJ / (mole °C)
e. None of the above
24. What is the ΔH for the combustion of
propane, C3H8?
a. -2010 kJ/mol
b. 2010 kJ/mol
c. -7 kJ/mol
d. 7 kJ/mol
e. None of the above
25. Which of the following conditions insures a
spontaneous reaction?
a. ΔH < 0
b. ΔS < 0
c. ΔG < 0
d. All of the above
e. None of the above
26. Which of the following is an accepted way of
determining the ΔH of a reaction?
a. Experimentally with calorimetery
b. Mathematically using bond energies
c. Mathematically using published ΔHf
values and Hess’ Law
d. All of the above
e. None of the above
27. If a reaction has a ΔH = 188 kJ/mole and
a ΔS = 3770 J / (mole K), at what temperature range would this reaction be
spontaneous?
a. T < 49.9 K
b. T > 49.9 K
c. T < 0.02 K
d. T > 0.02 K
e. None of the above
28.
If a chemical reaction is exothermic, energy is which of the following
in the reaction?
a. a
product
b. a
reactant
c. a
bystander
d. a
warm Spring day
29.
The change in enthalpy is indicated by which of the following?
a. ΔA
b. ΔB
c. ΔH
d. ΔZ
30. If the absolute entropy for O2(g)
is 126 J / (mole K), what is the ΔS for the combustion of C2H4(g)? Products are in the gas state.
a. -28.5 J / K
b. 28.5 J / K
c. -209 J / K
d. 209 J
/ K
e. None of the above
31. What does a bond strength of 602 kJ/mol for a
C=C mean?
a. It tells us the amount of energy required to
break 1 mole of C=C bonds.
b. It tells us how much energy will be absorbed
when 1 mole of C=C bonds are broken.
c. It tells us how much energy will be released
when 1 mole of C=C bonds are formed.
d. All of the above
e. None of the above
32. Potential
energy is defined as which of the following?
a.
stored energy
b.
motion energy
c.
canned energy
b.
bottled energy
33.
If the chemical reaction is endothermic, the entire reaction will
demonstrate which of the following?
a.
colder temperature
b.
higher pressure
c.
greater volume
d.
no change whatsoever
34. ΔH for all endothermic
reactions is which of the following?
a. positive
b. negative
c. a mythical value with can’t
be determined
d. playing quarterback for the
Seattle Seahawks
35. Which of the following are valid units for
bond strengths?
a. kJ/mole
b. kcals/g
c. mole/kcals
d. kcals/kJ
e. none of the above
36. Which of the following would definitely have
a higher entropy than a 50.0 g sample of CO2(g) at 56°C?
a. 25.0 g CO2 (g) at 60°C
b. 57.0 g CO2 (l) at 56°C
c. 25.0 g CO2 (l) at 50°C
d. 57.0 g CO2 (g) at 60°C
e. There is not enough information to answer
this problem.
37. Whose Law can be stated as, “Enthalpy is a
state function and is, therefore, independent of its path.”
a. Boyle’s
b. Chuck’s
c. Hess’s
d.
Wile’s
38.
In order for rearrangement of electrons to occur, they must be given
enough energy to overcome which of the following?
a. the
attraction that they feel toward each other
b.
the repulsion that they feel toward each other
c.
their Monday morning blahs
d.
their overnight sleepover fatigue
39.
If the Gibbs Free Energy value is consistent with the Second Law of
Thermodynamics, then the reaction is which of the following?
a.
free
b.
undecided
c.
spontaneous
d.
not spontaneous
40. A quantity that depends solely on the final
destination and not on the way you get to the destination is called a(n)
____________________.
a. inconclusive quantity
b. Hess’ Law
c. entropy
d. state function
e. none of the above
C. Calculations/Equations
- Calculate the answers to the following problems: 5 points each
(Be sure to show the correct units in your answer and balance any equations!)
41.
In order to make the shells that house and protect them, many shellfish
take solid lime (CaO) from the ocean floor and react it with gaseous carbon
dioxide that has been exhaled by marine organisms. The resulting calcium carbonate is the major
component of their shell. What is the
ΔH° for this reaction? (Use Table
13.2 in Appendix A)
42.
Ethane gas (C2H6) has also been considered as a
fuel for automobiles because, like octane, it releases a lot of energy when it
is burned. How many kJ of energy are
released when 250.0 grams of ethane undergo complete combustion? (Use Table 13.2 in Appendix A)
_____ points earned /50 points total x 100
= _____ %