What current will deposit 3.25g of zinc in 2hrs? [Zn = 65, F = 96500 mol-]

To find the current required to deposit 3.25g of zinc in 2 hours, we need to use Faraday's laws of electrolysis which states that the mass of substance deposited during electrolysis is directly proportional to the quantity of electricity passed through it. We can use the formula: Mass of substance = (Current × Time × Atomic weight) / (96500 × Valency) where the atomic weight and valency are taken from the chemical formula of the substance. For zinc, the atomic weight is 65 and the valency is 2. Plugging in the values given in the question, we get: 3.25 = (Current × 2 × 65) / (96500 × 2) Solving for the current, we get: Current = (3.25 × 96500 × 2) / (2 × 65 × 2) = 1340.38 A Rounding off to two significant figures, the answer is 1.3A. Therefore, the answer is: 1.34A.