The standard electrode potentials for some ha | vedclass

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(C) The standard reduction potential $(E^o)$ indicates the tendency of a species to get reduced. $A$ higher $E^o$ value means a stronger oxidizing age

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$Sn^{2+}$ is a stronger reducing agent than $Hg_{2}^{2+}$.

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(C) The standard reduction potential $(E^o)$ indicates the tendency of a species to get reduced. $A$ higher $E^o$ value means a stronger oxidizing agent and a weaker reducing agent.Comparing the given potentials:$E^o(PbO_2/Pb^{2+}) = +1.45 \ V$$E^o(Hg^{2+}/Hg_2^{2+}) = +0.92 \ V$$E^o(Sn^{4+}/Sn^{2+}) = +0.15 \ V$$1$. Reducing strength is the reverse of reduction potential. Since $E^o(Sn^{4+}/Sn^{2+}) $2$. Oxidizing strength follows the order of $E^o$ values: $PbO_2 > Hg^{2+} > Sn^{4+}$.Thus,$Sn^{2+}$ is a stronger reducing agent than $Hg_2^{2+}$.

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The standard electrode potentials for some half-reactions are given below. Which statement is correct?$(A) Sn^{4+} + 2e^{-} \rightarrow Sn^{2+}, E^o = +0.15 \ V$$(B) 2Hg^{2+} + 2e^{-} \rightarrow Hg_{2}^{2+}, E^o = +0.92 \ V$$(C) PbO_2 + 4H^{+} + 2e^{-} \rightarrow Pb^{2+} + 2H_2O, E^o = +1.45 \ V$