AP Chemistry Unit 9 focuses on electrochemistry, including galvanic and electrolytic cells, standard reduction potentials, and thermodynamic favorability of reactions. This resource provides multiple-choice questions designed for students preparing for the AP Chemistry exam. Each question challenges students to apply their understanding of key concepts, such as cell potentials and reaction mechanisms. Ideal for AP Chemistry students looking to reinforce their knowledge and practice exam-style questions.

Key Points

  • Covers electrochemistry concepts including galvanic and electrolytic cells.
  • Includes multiple-choice questions aligned with AP Chemistry curriculum.
  • Focuses on standard reduction potentials and thermodynamic principles.
  • Designed for students preparing for the AP Chemistry exam.
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AP Chemistry Scoring Guide
Unit 9 Progress Check: MCQ
Copyright © 2020. The College Board. These materials are part of a College Board program. Use or distribution of these materials online or in print
beyond your school’s participation in the program is prohibited.
Page 1 of 21
Table 1
Cell Type Operating Cell Potential for Commercial Batteries,
Lithium-iodine
Zinc-mercury
Table 2
Half-Reaction Standard Reduction Potential,
used to power pacemakers and have replaced zinc-mercury cells. Table 1 provides the operating cell potential, ,
for each cell. Table 2 provides the standard reduction potentials for several half-reactions related to zinc-mercury
and zinc-air cells.
1. Based on the information given, which of the following is a major difference between the zinc-mercury cell
and the lithium-iodine cell?
A
During the initial cell operation, each reaction is thermodynamically favorable, but the larger operating
potential of the lithium-iodine cell indicates that its cell reaction is less thermodynamically favorable.
B
During the initial cell operation, each reaction is thermodynamically favorable, but the larger operating
potential of the lithium-iodine cell indicates that its cell reaction is more thermodynamically favorable.
C
During the initial cell operation, the oxidation of iodine is thermodynamically favorable but the oxidation of
mercury is not.
D
During the initial cell operation, the oxidation of mercury is thermodynamically favorable but not the
oxidation of iodine is not.
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2. On average, after one year of operation, the potential of a lithium-iodine cell decreases by 1%-2%. Which of
the following best helps to explain the cause for the decrease in cell potential?
A
, and as the cell operates, decreases.
B
, and as the cell operates, increases.
C
, and as the cell operates, decreases.
D
, and as the cell operates, increases.
3.
The use of zinc-mercury cells in hearing aids has been replaced by zinc-air cells that operate using the
oxidation of by from the air, generating a potential of . Table 2 provides the standard
reduction potentials for the half-reactions used in zinc-mercury and zinc-air cells. Which of the following
best explains the modification to the cell design that is mostly responsible for the difference in standard cell
potentials for zinc-mercury and zinc-air cells?
A
The greater standard cell potential of the cell compared to that of the zinc-mercury cell most likely
results from the thermodynamically more favorable reduction of compared to .
B
The greater standard cell potential of the cell compared to that of the zinc-mercury cell most likely
results from the greater number of moles of required to reduce compared to .
C
The greater standard cell potential of the cell compared to that of the zinc-mercury cell most likely
results from the thermodynamically less favorable reduction of compared to .
D
The greater standard cell potential of the cell compared to that of the zinc-mercury cell most likely
results from the greater number of moles of hydroxide ions required to reduce compared to
.
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AP Chemistry Scoring Guide
Unit 9 Progress Check: MCQ
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beyond your school’s participation in the program is prohibited.
Page 3 of 21
4.
The diagrams above represent physical changes for potassium. Which of the following correctly identifies
the physical process and provides the correct for the process in the indicated diagram?
A
In diagram 1, the process is freezing and is negative.
B
In diagram 2, the process is melting and is negative.
C
In diagram 3, the process is boiling and is negative.
D
In diagram 4, the process is condensation and is positive.
5.
Two samples containing an equal number of moles of are kept inside separate 1-liter rigid containers.
The particle diagrams above show the distribution of molecular speeds in each sample. Based on the
information given, which of the following identifies the sample with the greater , and why?
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FAQs

What topics are covered in the AP Chemistry Unit 9 Progress Check?
The AP Chemistry Unit 9 Progress Check covers essential topics in electrochemistry, including the principles of galvanic and electrolytic cells. It explores standard reduction potentials and how they influence cell voltage. Additionally, the questions assess students' understanding of thermodynamic favorability and the relationship between reaction mechanisms and energy changes. This comprehensive approach ensures students are well-prepared for the AP exam.

How does the concept of cell potential relate to electrochemical cells?
Cell potential is a critical concept in electrochemistry that quantifies the driving force behind electron transfer in electrochemical cells. In galvanic cells, a positive cell potential indicates a spontaneous reaction, while in electrolytic cells, a negative cell potential signifies a non-spontaneous reaction that requires external energy. Understanding how to calculate and interpret cell potential is essential for predicting the behavior of electrochemical reactions and designing efficient energy systems.

What is the significance of standard reduction potentials in electrochemistry?
Standard reduction potentials provide a measure of the tendency of a chemical species to gain electrons and be reduced. These values are crucial for determining the feasibility of redox reactions and calculating the overall cell potential in electrochemical cells. By comparing standard reduction potentials, students can predict which reactions will occur spontaneously and understand the energy changes associated with electron transfer.

How do thermodynamic principles apply to electrochemical reactions?
Thermodynamic principles are fundamental in analyzing electrochemical reactions, particularly in understanding spontaneity and energy changes. The Gibbs free energy change is directly related to cell potential, allowing students to determine whether a reaction is thermodynamically favorable. By applying these principles, students can evaluate the efficiency of electrochemical processes and their applications in energy storage and conversion.