Discussion
What is the quantity of current required to deposit one mole of metallic magnesium from fused magnesium chloride? (1F=96500C)
Answer: E
The charge needed is \(1.93 \times 10^{5}\) C.
At the cathode, \(\mathrm{Mg^{2+} + 2e^{-} \rightarrow Mg}\), so one mole of magnesium needs two moles of electrons, that is 2 faradays:
\[ Q = 2 \times 96500 = 193000 = 1.93 \times 10^{5}\ \text{C} \]
\(9.65 \times 10^{4}\) C is one faraday, enough only for a univalent metal. The other options are these values with the wrong power of ten.
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