The $E^{\circ}$ values of half-cells are given below. Which combination of two half-cells will result in a cell with the maximum potential?
$(i) \, A^{3-} \rightarrow A^{2-} + e^{-}; E^{\circ} = 1.5 \, V$
$(ii) \, B^{+} + e^{-} \rightarrow B; E^{\circ} = 0.5 \, V$
$(iii) \, C^{2+} + e^{-} \rightarrow C^{+}; E^{\circ} = 0.5 \, V$
$(iv) \, D \rightarrow D^{2+} + 2e^{-}; E^{\circ} = -1.15 \, V$

  • A
    $(ii)$ and $(iii)$
  • B
    $(i)$ and $(iv)$
  • C
    $(ii)$ and $(iv)$
  • D
    $(iii)$ and $(iv)$

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Similar Questions

Given the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$

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Match the following:
List-$I$List-$II$
$(A)$ Potential of hydrogen electrode at $pH = 10$$(I)$ $0.76 \ V$
$(B)$ $Cu^{2+} | Cu$$(II)$ $0.059$
$(C)$ $Zn | Zn^{2+}$$(III)$ $-0.591 \ V$
$(D)$ $\frac{2.303 RT}{F}$$(IV)$ $0.337 \ V$
$(V)$ $-0.76 \ V$

$A$ $B$ $C$ $D$
$(a)$ $(III)$ $(I)$ $(II)$ $(V)$
$(b)$ $(II)$ $(V)$ $(I)$ $(IV)$
$(c)$ $(III)$ $(IV)$ $(I)$ $(II)$
$(d)$ $(V)$ $(I)$ $(IV)$ $(II)$

The reducing ability of the metals $K$,$Au$,$Zn$ and $Pb$ follows the order

$Mg^{2+}$ displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Mg/Mg^{2+}$ has an $EMF$ of $2.71 \ V$ at $298 \ K$. If the potential of copper electrode is $0.34 \ V$,what is the reduction potential of $Mg$ electrode?

Which of the following reactions exhibits the minimum standard reduction potential?

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