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| Sections | |||
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| Redox Reaction | 32 mins | 0 completed | Learn Summary |
| Balancing Redox Reaction | 31 mins | 0 completed | Learn |
| The Nernst Equation | 11 mins | 0 completed | Learn |
| Faraday's Constant | 10 mins | 0 completed | Learn |
| Galvanic Cell | 85 mins | 0 completed | Learn |
| Batteries and Electricity | 9 mins | 0 completed | Learn |
| Additional Practice |
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| Cell Notation |
| Standard Hydrogen Electrode |
| Cell Potential |
| Electroplating |
| Electrolysis of Water & Mixture of Ions |
| Additional Guides |
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| Nernst Equation |
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
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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