State Faraday's first law of electrolysis. How much charge in Faraday is required for the reduction of 1 mol of MnO\(_4^-\) to Mn\(^{2+}\)?
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- Faraday's law helps determine the amount of substance deposited during electrolysis based on the charge passed through the electrolyte.
- The number of electrons involved in the reduction or oxidation process is key to calculating the total charge.
Faraday's first law of electrolysis states that:
The amount of chemical reaction which occurs at any electrode during electrolysis is proportional to the quantity of electricity passed through the electrolyte.
The equation is:
\[
m = ZIt
\]
Where:
- \(m\) is the mass of the substance deposited,
- \(Z\) is the electrochemical equivalent,
- \(I\) is the current,
- \(t\) is the time.
For the reduction of 1 mole of MnO\(_4^-\) to Mn\(^{2+}\), the number of electrons required is 5 (because MnO\(_4^-\) is reduced to Mn\(^{2+}\) by gaining 5 electrons).
Thus, the charge required to reduce 1 mole of MnO\(_4^-\) to Mn\(^{2+}\) is given by:
\[
Q = n \times F = 5 \times 96500 = 482500 \, \text{Coulombs}.
\]
Therefore, the charge required for the reduction of 1 mole of MnO\(_4^-\) to Mn\(^{2+}\) is 482500 Coulombs.
