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At a given temperature, which metal can reduce zinc oxide (\mathrm{ZnO}) and form a stable oxide of its own?

Option: 1

Copper (Cu)

Option: 2

Aluminum (Al)

Option: 3

Silver (Ag)

Option: 4

Platinum (Pt)

Answers (1)


At a given temperature, aluminium \mathrm{(Al)} can reduce zinc oxide (\mathrm{ZnO}) and form a stable oxide of its own. This is because aluminium is a more reactive metal compared to zinc. The reaction between aluminium and zinc oxide can be represented as follows:

\mathrm{2 A l(s)+Z n O(s) \rightarrow A l_2 O_3(s)+Zn(s)}

In this reaction, aluminium (Al) acts as the reducing agent, while zinc oxide (\mathrm{ZnO}) is being reduced to zinc (\mathrm{Zn}). The stable oxide formed in this reaction is aluminium oxide \left(\mathrm{Al}_2 \mathrm{O}_3\right). The other metals listed, copper (\mathrm{Cu}), silver (Ag), and platinum (Pt), are not able to reduce zinc oxide (\mathrm{ZnO}) and form stable oxides of their own in this particular reaction.

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