Faraday's Constant Video Lessons

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Example: Gold can be plated out of a solution containing Au3+ based on the following half reaction: Au3+ (aq) + 3 e -  ---->  Au (s) a) What mass of gold is plated by a 41 minute flow of 6.8 A current?

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Example: A solution of Mn+5 is used to plate out Mn in an electrochemical cell. If a total of 1.13 g of Mn is plated out in a total time of 1600 seconds, what was the electrical current used? (MW of Mn is 54.94 g/mol)

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Example: If steady current of 15 amperes is provided by a stable voltage of 12 Volts for 600 seconds, answer each of the following questions. a)  Calculate the total charge that passes through the circuit in this time. b)  Calculate the total number of moles of electrons that pass through the circuit in this time. c)  Calculate the total amount of energy that passes through the circuit in this time. d)  Calculate the power that the battery provides during this process.    

Problem: About how many grams of Sn+2(aq) are formed when 2 A is run through the cell below for 3 hours?Sn+4(aq) I Sn+2(aq) II Pb2+(aq) I Pb(s)1) about 10 grams2) about 20 grams3) about 5 grams4) none, Sn+2(aq) is not formed in the reaction.

FREE Expert Solution

We’re being asked to calculate the mass of Sn2+(aq) are formed when 2 A is run through the cell below for 3 hours.

Sn4+(aq) I Sn2+(aq) II Pb2+(aq) I Pb(s)


Let’s first determine how many electrons are involved in the reaction:

When writing a cell notation, we use the following format – “as easy as ABC”

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Problem Details

About how many grams of Sn+2(aq) are formed when 2 A is run through the cell below for 3 hours?
Sn+4(aq) I Sn+2(aq) II Pb2+(aq) I Pb(s)

1) about 10 grams

2) about 20 grams

3) about 5 grams

4) none, Sn+2(aq) is not formed in the reaction.

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