1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reduction of NO-3 ion in an aqueous solution E° is + 0.96 V. Values of E° for some metal ions are given below V2+(aq)+2e- longrightarrow V; E° = -1.19 Vtt Fe3+(aq)+3e- longrightarrow Fe; E° = -0.04 V Au3+(aq)+3e- longrightarrow Au; E° = +1.40 V Hg2+(aq)+2e- longrightarrow Hg; E° = +0.86 V The pair(s) of metals that is/are oxidised by NO-3 in aqueous solution is (are)

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Q. For the reduction of $NO^-_3$ ion in an aqueous solution $E^\circ$ is
$+ \,0.96\, V$. Values of $E^\circ$ for some metal ions are given below
$\, V^{2+}(aq)+2e^- \longrightarrow V;\, \, \, \, \, E^\circ = -1.19\, Vtt$
$\, Fe^{3+}(aq)+3e^- \longrightarrow Fe;\, \, \, \, \, E^\circ = -0.04 V$
$ Au^{3+}(aq)+3e^- \longrightarrow Au;\, \, \, \, \, E^\circ = +1.40\, V$
$ Hg^{2+}(aq)+2e^- \longrightarrow Hg;\, \, \, \, \, E^\circ = +0.86 V$
The pair(s) of metals that is/are oxidised by $NO^-_3$ in aqueous solution is (are)

IIT JEEIIT JEE 2009Redox Reactions

Solution:

Metals with $E^\circ$ value less than 0.96 V will be able to reduce $NO^-_3$
in aqueous solution.Therefore, metals V ($E^\circ$ = - 1.19 V),
Fe ($E^\circ$ = - 0.04 V), Hg ($E^\circ$ = 0.86 V) will all reduce $NO^-_3$ but Au
($E^\circ$ = 1.40 V) cannot reduce $NO^-_3$ in aqueous solution.