Question:
Given :
$\mathrm{Co}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Co}^{2+} ; \mathrm{E}^{\circ}=+1.81 \mathrm{~V}$
$\mathrm{~Pb}^{4+}+2 \mathrm{e}-\mathrm{Pb}^{2+} ; \mathrm{E}^{\circ}=+1.67 \mathrm{~V}$
$\mathrm{Ce}^{4+}+\mathrm{e}^{-} \rightarrow \mathrm{Ce}^{3+} ; \mathrm{E}^{\circ}=+1.61 \mathrm{~V}$
$\mathrm{Bi}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Bi} ; \mathrm{E}^{\circ}=+0.20 \mathrm{~V}$
Oxidizing power of the species will increase in the order :
Correct Option: , 4
Solution:
$\mathrm{E}_{\text {Red }}^{\circ} \uparrow \Rightarrow$ oxidizing power $\uparrow$
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