The Faraday constant F is the amount of electric charge carried by one mole of electrons, and it is approximately equal to 96,485 C/mol coulombs per mole . It is a fundamental constant in electrochemistry and can be used to relate the amount of substance produced or consumed during electrolysis to the total charge passed through the cell.To calculate the Faraday constant from the experimental data of electrolysis of nickel II sulfate, we can use the following steps:1. Calculate the total charge Q passed through the cell during electrolysis:Q = current I time t Q = 2.0 A 2.5 hours 3600 seconds/hour = 18,000 C2. Determine the molar mass of nickel Ni :The molar mass of nickel is approximately 58.69 g/mol.3. Calculate the moles of nickel deposited on the cathode:moles of Ni = mass of Ni deposited / molar mass of Nimoles of Ni = 0.245 g / 58.69 g/mol 0.00417 mol4. Determine the number of electrons transferred in the redox reaction:For the reduction of nickel II ions to nickel metal, the balanced half-reaction is:Ni + 2e NiSo, 2 moles of electrons are transferred per mole of nickel.5. Calculate the total moles of electrons transferred during electrolysis:total moles of electrons = moles of Ni moles of electrons per mole of Nitotal moles of electrons = 0.00417 mol 2 = 0.00834 mol6. Finally, calculate the Faraday constant F using the total charge Q and the total moles of electrons:F = Q / total moles of electronsF 18,000 C / 0.00834 mol 215,827 C/molThe calculated Faraday constant from this experimental data is significantly higher than the accepted value of 96,485 C/mol. This discrepancy could be due to experimental errors, impurities in the electrolyte, or other factors affecting the electrolysis process. In practice, the Faraday constant is a well-established value, and it would not be determined from a single experiment like this. Instead, it would be used to calculate other quantities, such as the amount of substance produced or consumed during electrolysis.