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: A current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?A) 900 moleB) 9.3 x10-3 moleC) 4.6 x10-3 moleD) 1.6 x 10-4 moleE) 7.8 x 10-5 mole 

FREE Expert Solution
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FREE Expert Solution

We’re being asked to calculate the number of moles of Cl2 gas evolved from the oxidation of Cl-.

Given:

• current = 0.5 A

▪ Note that amperes (A) = charge/time = C/s

▪ Current = 0.5 C/s

• t = 30 minutes

▪ Since current is in C/s, we will have to convert time from min to s

• Faraday’s constant = 96,485 C/(mol e-)

▪ Constant found in books or on the internet


Let’s first determine how many electrons are involved when Cl2 is generated from the reaction:

88% (106 ratings)
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Problem Details

A current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?


A) 900 mole
B) 9.3 x10-3 mole
C) 4.6 x10-3 mole
D) 1.6 x 10-4 mole
E) 7.8 x 10-5 mole

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