Here is a precise question for the student to solve:A student performed an electroplating experiment of copper metal onto an electrode by passing a constant current of 1.5 A through a solution of copper(II) sulfate for 50 minutes. If the mass of the copper metal obtained was 1.23 grams, calculate the Faraday constant using the following formula: Faraday constant = (mass of substance plated x molar mass of substance) / (current x time)

Question

Here is a precise question for the student to solve:A student performed an electroplating experiment of copper metal onto an electrode by passing a constant current of 1.5 A through a solution of copper(II) sulfate for 50 minutes. If the mass of the copper metal obtained was 1.23 grams, calculate the Faraday constant using the following formul

Answer 1

To calculate the Faraday constant, we will use the given formula:Faraday constant =  mass of substance plated x molar mass of substance  /  current x time First, we need to gather the necessary information:Mass of copper plated = 1.23 gramsMolar mass of copper = 63.55 grams/mol  rounded to two decimal places Current = 1.5 ATime = 50 minutesNow, we need to convert the time from minutes to seconds, as the unit for current is in Amperes  Coulombs/second :50 minutes * 60 seconds/minute = 3000 secondsNow, we can plug in the values into the formula:Faraday constant =  1.23 grams x 63.55 grams/mol  /  1.5 A x 3000 seconds Faraday constant =  78.1605 grammol  /  4500 As Faraday constant  17.369 molAsThe calculated Faraday constant is approximately 17.369 molAs. However, the actual Faraday constant is known to be around 96,485 C/mol  Coulombs per mole . The discrepancy in the calculated value could be due to experimental errors or inaccuracies in the given data.