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# One industrial process has an energy consumption of $18.5 \mathrm{kWh} / \mathrm{kg}$ of $\mathrm{Mg}$. How many joules are required per mole $(1 \mathrm{kWh}=1$ kilowatt-hour $=$ $\left.3.6 \times 10^6 \mathrm{~J}\right)$? How does this energy compare with the energy of the following process?\begin{align*} \mathrm{MgCl}_2(\mathrm{~s}) \rightarrow \mathrm{Mg}(\mathrm{s})+\mathrm{Cl}_2(\mathrm{~g}) \end{align*}

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In this problem, we are tasked to solve 3 different problems per item. For (a), we are tasked to solve for the volume of sea water to obtain $1.00 \ \text{kg Mg}$ and the mass of lime must be precipitated from the calculated volume of sea water, (b) mass of metal produced in the cathode, the compound produced at anode, mass of the product produced, and number of Faradays produced, and (c) calculate the amount of energy required per mole, and compare the amount of energy to the process shown below.

$\ce{MgCl2(s) -> Mg(s) +Cl2(g)} \tag{1}$

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