A solution of AuCl₃(aq)is electrolyzed by passing 85.0 A of current for 17.6 min.What mass of gold plates out? A)61.1 g B)1.02 g C)183 g D)0.483 g E)290 g

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Quizplus · Accepted Answer

The mass of gold plated out can be calculated using Faraday's laws of electrolysis. The amount of substance deposited (or liberated) at an electrode during electrolysis is directly proportional to the quantity of electricity that passes through the electrolyte. The formula to calculate the mass (m) is given by: m = (ItM)/(nF), where I is the current in amperes, t is the time in seconds, M is the molar mass of the substance (for gold, Au, it's approximately 197 g/mol), n is the number of moles of electrons exchanged per mole of substance (for Au^3+ to Au, n=3), and F is Faraday's constant (approximately 96485 C/mol).First, convert the time from minutes to seconds: 17.6 min * 60 s/min = 1056 s.Then, plug in the values: m = (85.0 A * 1056 s * 197 g/mol) / (3 * 96485 C/mol) = 61.1 g.Therefore, the mass of gold plated out is 61.1 g.

A Solution of AuCl3(aq)is Electrolyzed by Passing 85

A Solution of AuCl₃(aq)is Electrolyzed by Passing 85