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Carbon cannot reduce the oxides of sodium, magnesium and aluminium to their respective metals. Why? Where are these metals placed in the reactivity series? How are these metals obtained from their ores? Take an example to explain the process of extraction along with chemical equations.
Oxides of Sodium, magnesium and aluminium are very strong oxides as these metals are very reactive but carbon is not a strong reducing agent, hence, it cannot reduce these metal oxides.
In the reactivity series, sodium, magnesium, and aluminium are placed in the upper portion which means these metals are very reactive in nature and carbon is less reactive.
Oxides of reactive metals are directly put for the electrolytic reduction process to obtain the pure metal.
Example: Electrolysis of Molten NaCl
Electrolysis involves the movement of ions to the electrode. Solid-state does not allow the movement of ions and unsuitable for electrolysis. When melted at high temperature, sodium chloride separates into sodium and chloride ions, so that, electrolysis can take place to form sodium atom and chlorine gas.
NaCl → Na +(l) + Cl–(l)
At Anode: Cl− → 1/2Cl2(g) + e −
At Cathode : Na+ +e− →Na (s)
Net Reaction is written as: $2Na +(l) + 2Cl–(l) → 2Na(l) + Cl_2(g)$
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