What number of moles of Cu 2+ will be deposited by 360 coulombs of electricity? [f = 96500 C mol -1]

The question is asking us to calculate the number of moles of Cu2+ that will be deposited by 360 coulombs of electricity. We are given a constant "f" which is 96500 C mol-1. To solve this problem, we need to use Faraday's laws of electrolysis which states that the mass of substance deposited during electrolysis is proportional to the quantity of electricity passed. The formula is: Mass of substance = (Current × Time × Atomic weight) / (No. of electrons × Faraday's constant) In this question, we are not given the current, time, or atomic weight, but we are given the quantity of electricity (360 C) and Faraday's constant (96500 C mol-1). The number of electrons involved in the reaction is 2 (from Cu2+), so we can rearrange the formula to solve for the number of moles of Cu2+: Number of moles of Cu2+ = (Quantity of electricity / (No. of electrons × Faraday's constant)) Substituting the values, we get: Number of moles of Cu2+ = (360 C / (2 × 96500 C mol-1)) Number of moles of Cu2+ = 1.87 × 10-3 mol Therefore, the answer is the second option: 1.87 x 10-3 mole.