What is the standard reduction potential of $Cu^{2+} \mid Cu_{(s)}$ if the $E^{\circ}$ of the following cell is $0.46 \ V$ (in $V$)?
$Cu_{(s)} \mid Cu_{(aq)}^{2+} \parallel Ag_{(aq)}^{+} \mid Ag_{(s)}$ ; $E_{Ag^{+} / Ag}^{\circ} = 0.80 \ V$
$Cu_{(s)} \mid Cu_{(aq)}^{2+} \parallel Ag_{(aq)}^{+} \mid Ag_{(s)}$ ; $E_{Ag^{+} / Ag}^{\circ} = 0.80 \ V$
- A$1.56$
- B$0.34$
- C$1.44$
- D$1.26$
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Standard potential of electrode reaction $Cu^{2+}_{(aq)} + 2e^{-} \rightarrow Cu_{(s)}$ is $+0.34 \ V$. What is the standard potential of the reaction $2Cu_{(s)} \rightarrow 2Cu^{2+}_{(aq)} + 4e^{-}$?
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View SolutionThe standard reduction potential at $298 \ K$ for the following half cells are given below :-
$NO_3^{-} + 4H^{+} + 3e^{-} \rightarrow NO_{(g)} + 2H_2O \quad E^0 = 0.97 \ V$
$V^{2+}_{(aq)} + 2e^{-} \rightarrow V_{(s)}$ $E^0 = -1.19 \ V$ $Fe^{3+}_{(aq)} + 3e^{-} \rightarrow Fe_{(s)}$ $E^0 = -0.04 \ V$ $Ag^{+}_{(aq)} + e^{-} \rightarrow Ag_{(s)}$ $E^0 = 0.80 \ V$ $Au^{3+}_{(aq)} + 3e^{-} \rightarrow Au_{(s)}$ $E^0 = 1.40 \ V$
The number of metal$(s)$ which will be oxidized by $NO_3^{-}$ in aqueous solution is $....$.
$NO_3^{-} + 4H^{+} + 3e^{-} \rightarrow NO_{(g)} + 2H_2O \quad E^0 = 0.97 \ V$
| $V^{2+}_{(aq)} + 2e^{-} \rightarrow V_{(s)}$ | $E^0 = -1.19 \ V$ |
| $Fe^{3+}_{(aq)} + 3e^{-} \rightarrow Fe_{(s)}$ | $E^0 = -0.04 \ V$ |
| $Ag^{+}_{(aq)} + e^{-} \rightarrow Ag_{(s)}$ | $E^0 = 0.80 \ V$ |
| $Au^{3+}_{(aq)} + 3e^{-} \rightarrow Au_{(s)}$ | $E^0 = 1.40 \ V$ |
The number of metal$(s)$ which will be oxidized by $NO_3^{-}$ in aqueous solution is $....$.
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View SolutionIf the half-cell reaction $A + e^- \to A^-$ has a large negative reduction potential,it follows that
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View SolutionFerrous ion $(Fe^{2+})$ can be oxidised by which of the following ions?
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