Final answer:
To calculate the mass of palladium produced, we used Faraday's law of electrolysis and the stoichiometry of the reduction reaction of palladium ions. The total charge passed through the solution is multiplied by the molar mass of palladium to obtain the final mass, which is approximately 3.18 grams. Option A is the correct answer.
Step-by-step explanation:
The question is asking us to calculate the mass of palladium produced from the reduction of palladium (II) ions during electrolysis. We are given the current passed through the solution (3.2 C/s) and the duration for which this current is passed (30 minutes). To find the mass, we need to use Faraday's law of electrolysis and the stoichiometry of the reaction involving the palladium ions.
Firstly, convert the time to seconds: 30 minutes = 30 * 60 seconds = 1800 seconds. The total charge (Q) that passes through the cell can be found by multiplying the current by the time: Q = Current (I) * Time (t) = 3.2 C/s * 1800 s = 5760 C.
Secondly, we need to understand the stoichiometry of the reaction. The reduction of palladium (II) ions to palladium metal is represented by the equation: Pd2+ (aq) + 2e- → Pd (s). This means that we require 2 moles of electrons to reduce 1 mole of Pd2+ ions. Thus, the number of moles (n) of palladium produced is given by the equation: n = Q / (2 * Faraday's constant).
To calculate the mass of palladium produced, we use the molar mass of palladium (106.42 g/mol) and the number of moles calculated in the previous step: Mass = n * Molar mass of Pd. Therefore, the final answer is Mass of palladium produced = (5760 C / (2 * 96485 C/mol) * 106.42 g/mol), which equals approximately 3.18g of palladium.
Given the options, the correct one is (a) 3.18g.