Carbon cannot reduce the oxides of sodium, magnesium and aluminium lo
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.
Answers
Answer:
The two metals are above carbon in the reactivity series and thus have a high affinity to oxygen than carbon does and thus cannot be reduced by it. ... Metals of high reactivity; such as sodium, calcium, magnesium, aluminium, etc. are extracted from their ores by electrolytic reduction
(OR)
According to the reactivity series, both sodium and magnesium as well as aluminium are more reactive than carbon as these elements are placed above carbon in reactivity series.
As a result, being less reactive in nature carbon is unable to reduce oxides of Na,Mg & Al.
Metals of high reactivity such as sodium, magnesium & aluminium etc. are extracted from their ores by electrolytic reduction (Electrolysis) method.
Example: Electrolysis of Molten NaCl
At Anode: Cl
−
→
2
1
Cl
2(g)
+e
−
At Cathode : Na
+
+e
−
→Na
(s)
Overall reaction: 2NaCl→2Na
(s)
+Cl
2(g)
Explanation:
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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.
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ANSWER
According to the reactivity series, both sodium and magnesium as well as aluminium are more reactive than carbon as these elements are placed above carbon in reactivity series.
As a result, being less reactive in nature carbon is unable to reduce oxides of Na,Mg & Al.
Metals of high reactivity such as sodium, magnesium & aluminium etc. are extracted from their ores by electrolytic reduction (Electrolysis) method.
Example: Electrolysis of Molten NaCl
At Anode: Cl− → 1/2Cl2(g) +e −
At Cathode : Na+ +e− →Na (s)
Overall reaction: 2NaCl→2Na (s) +Cl