The 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 $....$.
- A$1$
- B$2$
- C$3$
- D$4$
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View SolutionThe standard reduction potentials at $298 \ K$ for the following half-cell reactions are given below:
$Zn^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Zn_{(s)} : -0.762 \ V$
$Cr^{3+}_{(aq)} + 3e^{-} \rightleftharpoons Cr_{(s)} : -0.74 \ V$
$2H^{+}_{(aq)} + 2e^{-} \rightleftharpoons H_{2(g)} : 0.00 \ V$
$Fe^{3+}_{(aq)} + e^{-} \rightleftharpoons Fe^{2+}_{(aq)} : 0.77 \ V$
Which one of the following is the strongest reducing agent?
$Zn^{2+}_{(aq)} + 2e^{-} \rightleftharpoons Zn_{(s)} : -0.762 \ V$
$Cr^{3+}_{(aq)} + 3e^{-} \rightleftharpoons Cr_{(s)} : -0.74 \ V$
$2H^{+}_{(aq)} + 2e^{-} \rightleftharpoons H_{2(g)} : 0.00 \ V$
$Fe^{3+}_{(aq)} + e^{-} \rightleftharpoons Fe^{2+}_{(aq)} : 0.77 \ V$
Which one of the following is the strongest reducing agent?
Consider the following cell:
$Zn_{(s)} \mid Zn^{2+}_{(1M)} \parallel KCl_{(sat)} \mid Hg_2Cl_{2(paste)} \mid Hg$
$E^{\circ}_{cell} = 1.007 \ V$ and $E^{\circ}_{calomel} = 0.242 \ V$
What is the standard potential of $Zn$ (in $V$)?
$Zn_{(s)} \mid Zn^{2+}_{(1M)} \parallel KCl_{(sat)} \mid Hg_2Cl_{2(paste)} \mid Hg$
$E^{\circ}_{cell} = 1.007 \ V$ and $E^{\circ}_{calomel} = 0.242 \ V$
What is the standard potential of $Zn$ (in $V$)?
$MX$ is a sparingly soluble salt that follows the given solubility equilibrium at $298 \ K$: $MX_{(s)} \rightleftharpoons M^{+}_{(aq)} + X^{-}_{(aq)}$; $K_{sp} = 10^{-10}$. If the standard reduction potential for $M^{+}_{(aq)} + e^- \rightarrow M_{(s)}$ is $(E^{\ominus}_{M^{+}/M}) = 0.79 \ V$, then the value of the standard reduction potential for the metal/metal insoluble salt electrode $E^{\ominus}_{X^{-}/MX_{(s)}/M}$ is . . . . . . $mV$. (nearest integer) [Given: $\frac{2.303 RT}{F} = 0.059 \ V$]
DifficultJEE MAIN 2026
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