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(C) The strength of an oxidant is directly proportional to its standard reduction potential $(E^o_{red})$.Comparing the given $E^o$ values:$MnO_4^- (1

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$Sn^{2+}, MnO_4^-$

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(C) The strength of an oxidant is directly proportional to its standard reduction potential $(E^o_{red})$.Comparing the given $E^o$ values:$MnO_4^- (1.52 \ V) > Fe^{3+} (0.77 \ V) > I_2 (0.54 \ V) > Sn^{4+} (0.1 \ V)$.Thus,$MnO_4^-$ has the highest reduction potential and is the strongest oxidant.The strength of a reductant is inversely proportional to the reduction potential of its corresponding oxidized form.Looking at the reverse reactions (oxidation potentials):$Sn^{2+} 	o Sn^{4+} + 2e^-; E^o_{ox} = -0.1 \ V$$2I^- 	o I_2 + 2e^-; E^o_{ox} = -0.54 \ V$$Fe^{2+} 	o Fe^{3+} + e^-; E^o_{ox} = -0.77 \ V$$Mn^{2+} + 4H_2O 	o MnO_4^- + 8H^{+} + 5e^-; E^o_{ox} = -1.52 \ V$$Sn^{2+}$ has the highest oxidation potential (least negative),making it the strongest reductant.Therefore,the strongest reductant is $Sn^{2+}$ and the strongest oxidant is $MnO_4^-$.

Given are $E^o$ values for some half reactions:
$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$
$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$
$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
The strongest reducant and oxidant respectively are:

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Given are $E^o$ values for some half reactions:$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$The strongest reducant and oxidant respectively are: