The last step in the Dow process for the production of magnesium metal involves electrolysis of molten MgCl₂.(b) Do the high temperatures required to melt MgCl2 favor products or reactants? (Hint: Consider the \Delta H_{\mathrm{f}}^{\circ} of MgCl₂.)

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23-08-2022
Chemistry

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The last step in the Dow process for the production of magnesium metal involves electrolysis of molten MgCl₂.(b) Do the high temperatures required to melt MgCl2 favor products or reactants? (Hint: Consider the \Delta H_{\mathrm{f}}^{\circ} of MgCl₂.)

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tripatsingh039 tripatsingh039 · Answer 1 · 2022-08-26T14:38:50+02:00

At high temperature, the reactants i.e. Mg metal and chlorine gas will be favoured.

An exothermic reaction is one in which the formation of new bonds in the products releases more energy than is required to break bonds in the reactants. Energy is continuously released during an exothermic reaction, frequently in the form of heat. Exothermic reactions characterize all combustion processes.

The formation of MgCl2 is an exothermic process. Its enthalpy of formation is -641.6 kJ/mol which is negative.

The reaction is

Mg(s)+ Cl2(g) → MgCl₂ (s)

The exothermic reaction is favoured by a decrease in temperature while its reverse reaction will be favoured by an increase in temperature.

Hence, at high temperature, the reactants i.e. Mg metal and chlorine gas will be favoured.

Learn more about the exothermic reaction here:

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