Question

Calculate the mass of (a) silver (b) copper (c) aluminum that will be deposited during electrolysis by the passage of 965 C of electricity (Cu = 64, Ag = 108, Al = 27, Faraday's constant = 96500 C mol^−1).

Answer 1

The mass of silver, copper, and aluminum deposited during electrolysis can be calculated using Faraday's law, which relates the charge passed through the cell to the amount of substance deposited. For silver, the mass is 1.08 g, for copper it is 0.64 g, and for aluminum it is 0.27 g.

Step-by-step explanation:

To calculate the mass of a substance deposited during electrolysis, we need to use Faraday's law. According to Faraday's law, the amount of substance deposited is directly proportional to the charge passed through the cell. The formula to calculate the mass is:

Mass = (Charge / Faraday's constant) x molar mass

a) For silver (Ag), Mass = (965 C / 96500 C mol⁻¹) x 108 g/mol = 1.08 g

b) For copper (Cu), Mass = (965 C / 96500 C mol⁻¹) x 64 g/mol = 0.64 g

c) For aluminum (Al), Mass = (965 C / 96500 C mol⁻¹) x 27 g/mol = 0.27 g

Answer 2

To calculate the mass of metal deposited during electrolysis, you can use Faraday's law. The formula involves the current, time, atomic mass, charge on one electron, and Faraday's constant. For silver, copper, and aluminum, the mass can be calculated using the respective atomic masses and the given amounts of electricity passed.

Step-by-step explanation:

The mass of the metal deposited during electrolysis can be calculated using Faraday's law. According to Faraday's law, the amount of a substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The formula is:

Mass (in grams) = (Current (in amperes) × Time (in seconds) × Atomic mass) / (Charge on one electron × Faraday's constant)

(a) For silver (Ag): Mass of Ag = (965 C × 108 g/mol) / (1.602 × 10^-19 C × 96500 C/mol)

(b) For copper (Cu): Mass of Cu = (965 C × 64 g/mol) / (1.602 × 10^-19 C × 96500 C/mol)

(c) For aluminum (Al): Mass of Al = (965 C × 27 g/mol) / (1.602 × 10^-19 C × 96500 C/mol)