Experiment 8: Electrochemistry I - Galvanic and Electrolytic Cells

What is the purpose of constructing galvanic and electrolytic cells in this experiment?

To explore spontaneous and non-spontaneous electrochemical reactions and experimentally determine Faraday's constant using copper electrodes.

What are the two main types of electrochemical cells mentioned in the notes?

Galvanic cells and electrolytic cells.

What type of reaction do galvanic cells use to produce electricity?

Spontaneous redox reactions.

In galvanic cells, where is the anode located?

On the left side.

What does a salt bridge do in an electrochemical cell?

Maintains charge neutrality by allowing ion flow.

What does the line notation represent in electrochemical cells?

It represents the components of the cell, with the anode on the left and cathode on the right.

What is the key equation for calculating cell potential?

E°cell = E°cathode − E°anode.

How is Faraday's constant related to electrolysis?

It relates the amount of substance deposited or dissolved to the current and time.

What does the equation Q = I × t represent?

It represents the total charge transferred in coulombs.

In the context of the experiment, what does 'non-spontaneous reaction' mean?

A reaction that requires an external voltage to occur.

What is the significance of measuring mass changes in electrodes during electrolysis?

To determine Faraday's constant.

What is the expected average value of Faraday’s constant?

Approximately 96485 C/mol e⁻.

What are two visual changes you might record in Part A of the experiment?

Changes in color or formation of solid precipitates.

Why would comparing observed voltages to theoretical voltages be necessary?

To calculate % error and validate the experiment's accuracy.

What does a discrepancy in observed vs theoretical values indicate?

Possible impurities or inaccuracies in the experimental setup.

What is the role of copper sulfate solution in the electrolytic cell?

It provides copper ions for the electrolysis process.

What happens to mass at the electrodes during electrolysis?

Mass is gained at the cathode and lost at the anode.

What are the three metal samples used in Part A of the experiment?

Copper (Cu), lead (Pb), and zinc (Zn).

Why might Fe electrodes yield less accurate results compared to Cu electrodes?

Potential contamination or different reactivity influencing the results.

How is the average and standard deviation of Faraday’s constant determined in this experiment?

By conducting multiple trials and calculating from each trial’s data.