Question
Download Solution PDFA solution of Ni(NO3)2 is electrolysed between Pt - electrodes using 0.1 Faraday electricity. How many moles of Ni will be deposited at the cathode?
Answer (Detailed Solution Below)
Detailed Solution
Download Solution PDFCONCEPT:
Electrolysis and Faraday’s Laws
- According to Faraday’s First Law of Electrolysis, the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity (in Faradays) passed through the electrolyte.
- The number of moles of a metal deposited is given by:
\(\text{Moles deposited} = \frac{\text{Electricity (Faradays)}}{\text{n-factor of metal}}\), - where "n-factor" is the number of electrons involved per ion in the reduction process.
EXPLANATION:
- For Ni2+ in the solution, the reduction reaction is:
\(\text{Ni}^{2+} + 2e^- \rightarrow \text{Ni (s)}\) - The n-factor for Ni is 2 because it requires 2 electrons to reduce Ni2+ to Ni (s).
- Given that 0.1 Faraday of electricity is used:
- Moles of Ni deposited = \(\frac{0.1}{2} = 0.05 \, \text{moles}\)
The correct answer is 0.05.
Last updated on May 30, 2025
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