    Question

# For the reduction of NO⊖3 ion in an aqueous solution, E⊖ is +0.96 V, the values of E⊖ for some metal ions are given below: (i)V2+(aq)+2e−→V; E⊖=−1.19V (ii)Fe3+(aq)+3e−→Fe; E⊖=−0.04V (iii)Au3+(aq)+3e−→Au; E⊖=+1.40V (iv)Hg2+(aq)+2e−→Hg; E⊖=+0.86V The pair(s) of metals that is/are oxidized by NO⊖3 in aqueous solution is/are (IIT-JEE, 2010)

A

Fe and Au

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B

Hg and Fe

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C

V and Hg

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D

Fe and V

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Solution

## The correct options are B Hg and Fe C V and Hg D Fe and V The basic idea is pretty straightforward here. You need to see if a reaction is spontaneous or not. How do you do this? Calculate the overall E0 of the reaction. If it is +ve, then the reaction would be spontanoues. Easy enough? You just need to check with every option since this is a multiple answer correct question. NO⊖3+e−→?;E⊖red=0.96V Compare the standard reduction potential fo the given metals with that of NO⊖3 reduction. E⊖reduction for NO⊖3 is greater than E⊖reduction of (i), (ii), and (iv). So, NO⊖3 will be able to oxidize Fe, Hg, and V. So pairs are as in (b), (c) and (d).  Suggest Corrections  0      Explore more