Lesson: The Faraday Constant Chemistry • 10th Grade

In this lesson, we will learn how to use the Faraday constant to calculate the mass or volume of substances liberated during electrolysis.

Lesson Plan

Students will be able to

explain the relationship between charge, current, and time,
link electricity and simple electrical laws to the Avogadro constant,
explain the Faraday constant in terms of the Avogadro constant and the charge on one electron,
use the quantity of charge passed to calculate the mass or volume of substance liberated.

Lesson Presentation

Lesson Video

Lesson Explainer

Lesson Flashcards

Equivalent weight (gram equivalent)

Lesson Worksheet

Q1:

What is the charge of a mole of electrons? The charge of a single electron is C .

Q2:

The reduction of aluminum ions is described by the ionic half-equation []

What charge, to 2 decimal places and in scientific notation, must be delivered to reduce 200 kg of aluminum ions to aluminum metal? The charge of a single electron is C.

Q3:

The reduction of lithium ions can be represented by the ionic half-equation []

How many electrons are required per lithium ion to produce lithium metal?

How many moles of electrons are required to reduce 1.00 g of lithium ions? Give your answer to the nearest 2 decimal places.

How much charge must be delivered to reduce 1.00 g of lithium ions? The charge of a single electron is C. Give your answer to the nearest 2 decimal places in scientific notation.