Question Video: Identifying the Defintion of the Faraday Constant | Nagwa Question Video: Identifying the Defintion of the Faraday Constant | Nagwa

Question Video: Identifying the Defintion of the Faraday Constant Chemistry • Third Year of Secondary School

Which of the following best defines the Faraday constant, 𝐹? [A] The amount of charge per mole of elementary charge [B] The number of electrons per mole of elementary charge [C] The mass of substance deposited at an electrode per coulomb of charge [D] The time taken to deliver one mole of electrons at an electrode [E] The flow of electric charge per second

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Video Transcript

Which of the following best defines the Faraday constant, 𝐹? (A) The amount of charge per mole of elementary charge. (B) The number of electrons per mole of elementary charge. (C) The mass of substance deposited at an electrode per coulomb of charge. (D) The time taken to deliver one mole of electrons at an electrode. Or (E) the flow of electric charge per second.

Say we have electrons traveling through a wire. We may know how much charge traveled through the circuit. But we want to know how many electrons were responsible for that charge. Faraday’s constant allows us to convert between these two quantities. Mathematically, Faraday’s constant has a value equal to Avogadro’s number multiplied by the elementary charge. Avogadro’s constant has a value of 6.022 times 10 to the 23 entities per mole. In this case, the entities are charged particles. Now what is the elementary charge?

Well, the proton has a charge of 1.602 times 10 to the negative 19 coulombs. This quantity of charge is called the elementary charge. Of course, the charge of the electron is exactly the opposite of the charge of the proton. So we can use the elementary charge in calculations involving the electron as well.

So, if we multiply Avogadro’s constant by the value of the elementary charge, we’ll be able to calculate Faraday’s constant, which we can calculate to be 96,472.4 coulombs per mole, using these rounded values. Usually, a rounded value of 96,500 columns per mole is used in calculations. So there’s about 96,500 coulombs of charge per mole of elementary charges. This matches answer choice (A). In other words, for every one mole of elementary charge transferred in a circuit, there are 96,500 coulombs of charge transferred.

So the statement that best defines Faraday’s constant is statement (A), the amount of charge per mole of elementary charges.

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