A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours. How many moles of calcium metal should be deposited

Question

Quizplus · Accepted Answer

First, we need to use Faraday's Law of Electrolysis to calculate the number of moles of calcium deposited:

moles of calcium = (current in amperes x time in seconds) / (Faraday's constant x charge on calcium ion)

Note that we need to convert the current from amperes to coulombs per second, and the time from hours to seconds:

current = 2.50 A = 2.50 C/s
time = 4.50 hours x 3600 s/hour = 16200 s

The Faraday constant is 96485 C/mol, and the charge on the calcium ion is 2+, so we have:

moles of calcium = (2.50 C/s x 16200 s) / (96485 C/mol x 2) = 0.210 mol

Therefore, the answer is B) 0.210 mol.

A Current of 2