Calculate the quantity of electricity that would be required to reduce 12.3 g of nitrobenzene to aniline if current efficiency is 50% and the potential drop across the cell is 3.0 volts.
Correct answer: B. 115800 coulombs
- A. 369000 coulombs
- B. 115800 coulombs
- C. 32100 coulombs
- D. 521900 coulombs
Explanation
To calculate the quantity of electricity, we use Faraday's law of electrolysis: Q = n × F, where Q is the quantity of electricity in coulombs, n is the number of moles of electrons, and F is Faraday's constant (approximately 96500 C/mol). Calculate the number of moles of nitrobenzene being reduced, considering the molar mass of nitrobenzene and the stoichiometry of the reduction reaction to aniline.Given the mass of nitrobenzene is 12.3 g, convert this to moles. Then, calculate the moles of electrons needed for the reduction reaction. Consider the 50% current efficiency, which indicates that only half of the electricity will actually be effective in the reaction.The correct quantity of electricity required is 115800 coulombs. Options A, C, and D either do not correctly apply Faraday's law or miscalculate the efficiency factor.
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