How many coulombs of charge are required to deposit 1.00 g Ag from a solution of Ag⁺(aq)?
To determine the number of coulombs of charge required to deposit 1.00 g of Ag from a solution of Ag⁺(aq), you need to follow these steps:
1. Calculate the moles of Ag in 1.00 g using the molar mass of Ag (107.87 g/mol). The formula is:
Moles = Mass / Molar mass
Moles = 1.00 g / 107.87 g/mol
2. Determine the number of electrons involved in the deposition of each Ag atom. Since Ag⁺(aq) is being reduced to Ag(s), one electron is required for each Ag⁺ ion.
3. Convert the number of moles of Ag to the number of Ag⁺ ions. Since each Ag⁺ ion requires one electron, the number of Ag⁺ ions is equal to the number of moles of Ag.
4. Finally, calculate the total number of coulombs using Faraday's constant, which is equal to 96,485 C/mol of electrons. The formula is:
Coulombs = Number of moles of Ag⁺ ions × Faraday's constant
By following these steps, you can determine the number of coulombs of charge required to deposit 1.00 g Ag from a solution of Ag⁺(aq).