Answer:
Since there is no change in the oxidation states of any element involved in the reaction, we can conclude that this is not a redox reaction.
Step-by-step explanation:
To determine if the given reaction is a redox reaction, we need to identify the changes in oxidation states of the elements involved.
We know that:
Oxidation state of Na in NaCl(aq) is +1.
Oxidation state of Cl in NaCl(aq) is -1.
Oxidation state of Pb in PbO2(aq) is +4.
Oxidation state of O in PbO2(aq) is -2.
Oxidation state of Na in Na2O(aq) is +1.
Oxidation state of O in Na2O(aq) is -2.
Oxidation state of Pb in PbCl4(aq) is +4.
Oxidation state of Cl in PbCl4(aq) is -1.
By comparing the oxidation states of the elements before and after the reaction, we can observe that the oxidation state of Pb has increased from +4 to +4. Therefore, Pb has not undergone any change in oxidation state.
The oxidation state of Cl has also remained from -1 to -1. Hence, Cl has also not undergone any change in oxidation state.
Hence, we can conclude that this is not a redox reaction.