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
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:

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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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