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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Similar Questions
The standard electrode potentials at $25\,^oC$ for the following half-reactions are given:
$Zn^{2+} + 2e^- \to Zn, E^o = -0.762\,V$
$Mg^{2+} + 2e^- \to Mg, E^o = -2.37\,V$
When zinc dust is added to a solution of $MgCl_2$,what happens?
$Zn^{2+} + 2e^- \to Zn, E^o = -0.762\,V$
$Mg^{2+} + 2e^- \to Mg, E^o = -2.37\,V$
When zinc dust is added to a solution of $MgCl_2$,what happens?
Difficult
View SolutionMatch the following:
List-$I$ List-$II$ $(A)$ Potential of hydrogen electrode at $pH = 10$ $(I)$ $0.76 \ V$ $(B)$ $Cu^{2+} | Cu$ $(II)$ $0.059$ $(C)$ $Zn | Zn^{2+}$ $(III)$ $-0.591 \ V$ $(D)$ $\frac{2.303 RT}{F}$ $(IV)$ $0.337 \ V$ $(V)$ $-0.76 \ V$
$A$ $B$ $C$ $D$
$(a)$ $(III)$ $(I)$ $(II)$ $(V)$
$(b)$ $(II)$ $(V)$ $(I)$ $(IV)$
$(c)$ $(III)$ $(IV)$ $(I)$ $(II)$
$(d)$ $(V)$ $(I)$ $(IV)$ $(II)$
| List-$I$ | List-$II$ |
|---|---|
| $(A)$ Potential of hydrogen electrode at $pH = 10$ | $(I)$ $0.76 \ V$ |
| $(B)$ $Cu^{2+} | Cu$ | $(II)$ $0.059$ |
| $(C)$ $Zn | Zn^{2+}$ | $(III)$ $-0.591 \ V$ |
| $(D)$ $\frac{2.303 RT}{F}$ | $(IV)$ $0.337 \ V$ |
| $(V)$ $-0.76 \ V$ |
$A$ $B$ $C$ $D$
$(a)$ $(III)$ $(I)$ $(II)$ $(V)$
$(b)$ $(II)$ $(V)$ $(I)$ $(IV)$
$(c)$ $(III)$ $(IV)$ $(I)$ $(II)$
$(d)$ $(V)$ $(I)$ $(IV)$ $(II)$
Four metals $A$,$B$,$C$,and $D$ have Standard Reduction Potential $(SRP)$ values of $-3.05 \ V$,$-1.66 \ V$,$-0.40 \ V$,and $0.80 \ V$ respectively. Which is the strongest reducing agent?
Medium
View SolutionArrange the following metals in the order in which they displace each other from the solution of their salts: $Al$,$Cu$,$Fe$,$Mg$,and $Zn$.
Medium
View SolutionAmong the following metals,the strongest reducing agent is
DifficultKVPY 2017
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