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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.

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