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For the reduction of NO(3)^(-) in an aqu...

For the reduction of `NO_(3)^(-)` in an aqueous solution, `E^(@)` is 0.96V. Values of `E^(@)` for some metal ions are given below
`V_((aq))^(2+) + 2e^(-) rarr V E^(@) = -1.19V`
`Fe_((aq))^(3+) + 3e^(-) rarr Fe E^(@)= -0.04V`
`Au_((aq))^(3+) + 3e^(-) rarr Au E^(@)= +1.40V`
`Hg_((aq))^(2+) + 2e^(-) rarr Hg E^(@)= +0.86V`
The pair(s) of metal that is (are) oxidised by `NO_(3)^(-)` in aqueous solution is (are)

A

V and Hg

B

Hg and Fe

C

Fe and Au

D

Fe and V

Text Solution

Verified by Experts

The correct Answer is:
A, B, D
`E_M^(n+)//M)^(@)` for V, Fe, Hg are lower than that of `NO_(3)^(-)`. So, `NO_(3)^(-)` will oxidised V, Fe and Hg
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