For the reduction of NO3− ion in an aqueous solution , E0 is +0.96V. Values of E0 for some metal ions are given below V2+(aq)+2e−→V E0=−1.19V Fe3+(aq)+3r−→Fe E0=−0.04V Au3+(aq)+3e−→Au E0=+1.40V Hg2+(aq)+2e−→Hg E0=+0.86V The pair(s) of metals that is (are) oxidized by NO3− in aqueous solution is(are)

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For the reduction of {N}{{O}_{{{3}}}^{{-}}} ion in an aqueous

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For the reduction of $N O_{3}^{-}$ ion in an aqueous solution , $E^{0}$ is +0.96V. Values of $E^{0}$ for some metal ions are given below
$V^{2 +} (a q) + 2 e^{-} \to V E^{0} = - 1.19 V$
$F e^{3 +} (a q) + 3 r^{-} \to F e E^{0} = - 0.04 V$
$A u^{3 +} (a q) + 3 e^{-} \to A u E^{0} = + 1.40 V$
$H g^{2 +} (a q) + 2 e^{-} \to H g E^{0} = + 0.86 V$
The pair(s) of metals that is (are) oxidized by $N O_{3}^{-}$ in aqueous solution is(are)

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For the reduction of

N O_{3}^{-}

ion in an aqueous solution ,

E^{0}

is +0.96V. Values of

E^{0}

for some metal ions are given below

V^{2 +} (a q) + 2 e^{-} \to V E^{0} = - 1.19 V

F e^{3 +} (a q) + 3 r^{-} \to F e E^{0} = - 0.04 V

A u^{3 +} (a q) + 3 e^{-} \to A u E^{0} = + 1.40 V

H g^{2 +} (a q) + 2 e^{-} \to H g E^{0} = + 0.86 V

The pair(s) of metals that is (are) oxidized by

N O_{3}^{-}

in aqueous solution is(are)

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