Lesson: The Faraday Constant

Chemistry

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

Sample Question Videos

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02:27

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 [ = 27 g/mol]

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 [ = 7 g/mol]

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.

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