$PbO$ and $PbO_2$ react with $HCl$ according to the following chemical equations:
$(i)$ $2PbO + 4HCl \to 2PbCl_2 + 2H_2O$
$(ii)$ $PbO_2 + 4HCl \to PbCl_2 + Cl_2 + 2H_2O$
Why do these compounds differ in their reactivity?
$(i)$ $2PbO + 4HCl \to 2PbCl_2 + 2H_2O$
$(ii)$ $PbO_2 + 4HCl \to PbCl_2 + Cl_2 + 2H_2O$
Why do these compounds differ in their reactivity?
(N/A) In equation $(i)$,the oxidation number of the elements does not change,so this reaction is not a redox reaction. It is an acid-base reaction.
In equation $(ii)$,the oxidation number of $Pb$ decreases from $+4$ to $+2$ (reduction) and the oxidation number of $Cl$ increases from $-1$ to $0$ (oxidation). Thus,$PbO_2$ acts as an oxidising agent and $Cl^-$ is oxidised to $Cl_2$.
In equation $(ii)$,the oxidation number of $Pb$ decreases from $+4$ to $+2$ (reduction) and the oxidation number of $Cl$ increases from $-1$ to $0$ (oxidation). Thus,$PbO_2$ acts as an oxidising agent and $Cl^-$ is oxidised to $Cl_2$.
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| List-$I$ (Reaction) | List-$II$ (Type of redox reaction) |
| $A$. $N_{2(g)} + O_{2(g)} \rightarrow 2 NO_{(g)}$ | $I$. Decomposition |
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Choose the correct answer from the options given below:
Which of the following reactions is not a redox reaction?
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