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Question
\[\ce{PbO}\] and \[\ce{PbO2}\] react with \[\ce{HCl}] according to following chemical equations:
\[\ce{2PbO + 4HCl -> 2PbCl2 + 2H2O}\]
\[\ce{PbO2 + 4HCl -> PbCl2 + Cl2 + 2H2O}\]
Why do these compounds differ in their reactivity?
Solution
\[\ce{2PbO + 4HCl -> 2PbCl2 + 2H2O}\] (Acid base reaction)
\[\ce{PbO2 + 4HCl -> PbCl2 + Cl2 + 2H2O}\] (Redox reaction)
In reaction (i), O.N. of none of the atoms undergo a change. Therefore, it is not a redox reaction. It is an acid-base reaction, because \[\ce{PbO}\] is a basic oxide which reacts with \[\ce{HCl}\] acid.
The reaction (ii) is a redox reaction in which \[\ce{PbO2}\] gets reduced and acts as an oxidizing agent.
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