A current of 12.0 A is passed through molten magnesium chloride for 14.0 h.How many moles of magnesium metal can be produced from this electrolysis?
A) 0.0522 mol
B) 3.13 mol
C) 0.37 mol
D) 0.22 mol
E) 6.27 mol

Question

Quizplus · Accepted Answer

The amount of magnesium produced can be calculated using Faraday's laws of electrolysis. The charge passed through the electrolyte is given by $Q = I \times t$, where $I$ is the current (12.0 A) and $t$ is the time in seconds (14.0 h \times 3600 s/h = 50400 s). Thus, $Q = 12.0 A \times 50400 s = 604800 C$. The molar charge required to deposit one mole of magnesium (Mg) is given by $nF$, where $n$ is the number of moles of electrons required to deposit one mole of Mg (2 moles of electrons for Mg, since Mg has a valency of 2) and $F$ is Faraday's constant ($96485 C/mol$). Therefore, the moles of Mg produced are $Q / (nF) = 604800 C / (2 \times 96485 C/mol) = 3.13 mol$.

A Current of 12