What is the standard value of Faraday's constant used in electrochemistry?

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Multiple Choice

What is the standard value of Faraday's constant used in electrochemistry?

Explanation:
Faraday's constant is the amount of electric charge carried by one mole of electrons. It comes from multiplying the elementary charge by Avogadro's number: F = NA × e. Using e ≈ 1.6022×10^-19 C and NA ≈ 6.022×10^23 mol^-1 gives F ≈ 9.6485×10^4 C/mol. In electrochemistry this lets us relate total charge to moles of electrons transferred via Q = nF. The standard value used is about 96485 C per mole of electrons, commonly written as 96485 C/mol. The other numbers are from different constants: 1000 C/mol is just a rough approximation; 8.314 J/mol-K is the gas constant; 6.022×10^23 mol^-1 is Avogadro's number, the quantity of particles per mole, not a charge.

Faraday's constant is the amount of electric charge carried by one mole of electrons. It comes from multiplying the elementary charge by Avogadro's number: F = NA × e. Using e ≈ 1.6022×10^-19 C and NA ≈ 6.022×10^23 mol^-1 gives F ≈ 9.6485×10^4 C/mol. In electrochemistry this lets us relate total charge to moles of electrons transferred via Q = nF. The standard value used is about 96485 C per mole of electrons, commonly written as 96485 C/mol. The other numbers are from different constants: 1000 C/mol is just a rough approximation; 8.314 J/mol-K is the gas constant; 6.022×10^23 mol^-1 is Avogadro's number, the quantity of particles per mole, not a charge.

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