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

For the reduction of `NO_(3)^(-)` ion in an aqueous solution `E^(@)` is `+0.96V`. Values of `E^(@)` for some metal ions are given below `V^(2+)(aq)+2e^(-)hArrV,E^(@)=-1.19V t t`
`Fe^(3+)(aq)+3e^(-)rarrFe: E^(@)=-0.04V`
`Au^(3+)(aq)+3e^(-)rarrAu, E^(@)=+1.40V`
`Hg^(2+)(aq)+3e^(-)rarrHg, E^(@)=+0.86V`
The pari(s) of metals that is/are oxidised by `NO_(3)^(-)` in aqueous solution is (are)

V and Hg

Hg and Fe

Fe and Au

Fe and V

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The correct Answer is:

a,b,d

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For the reduction of NO_(3)^(-) ion in an aqueous solution E^(@) is +0.96V . Value of E^(@) for some metal ions are given below V^(2+)(aq)+2e^(-)rarrV E^(@)=-1.19V Fe^(3+)(aq)+3e^(-)rarrFe E^(@)=-0.04V Au^(3+)(aq)+3e^(-)rarrAu E^(@)=+1.40V Hg^(2+)(aq)+2e^(-)rarrHg E^(@)=+0.86V The pair(s) of metal that is/are oxidised by NO_(3)^(-) in aqueous solution is(arE):

For the reduction of NO_(3)^(-) ion in an aqueous solution, is +0.96V. Values of for some metal ions are given below : V^(2+)(aq)+ 2e^(-)rightarrowV , E^(@)= -1.19V Fe^(3+)(aq)+ 3e^(-) rightarrow Fe , E^(@) = -0.04 V Au^(3+)(aq) + 3e^(-) rightarrow Au , E^(@) = +1.40V Hg^(2+) (aq)+ 2e^(-) rightarrowHg , E^(@) = + 0.86 V The pair(s) of metals that is(are) oxidised by NO_(3)^(-) in aqueous solution is(are) :

For the reduction of NO_(3)^(c-) ion in an aqueous solution, E^(c-) is +0.96V , the values of E^(c-) for some metal ions are given below : i.V^(2+)(aq)+2e^(-)rarr V, " "E^(c-)=-1.19V ii. Fe^(3+)(aq)+3e^(-) rarr Fe, " "E^(c-)=-0.04V iii. Au^(3+)(aq)+3e^(-) rarr Au, " "E^(c-)=+140V iv. Hg^(2+)(aq)+2e^(-) rarr Hg, " "E^(c-)=+0.86V The pair (s) of metals that is // are oxidized by NO_(3)^(c-) in aqueous solution is // are

Electrode potential data are given below {:(Fe^(3+)(aq)+e^(-)rarrFe^(2+)(aq),E^(@)=+0.77V),(Al^(3+)(aq)+3e^(-)rarrAl(s),E^(@)=-1.66V),(Br_(2)(aq)+2e^(-)rarrBr^(-)(aq),E^(@)=+1.05V):} Based on the given data which statements is/are true?

The standard reduction potentials at 298K, for the following half cells are given: Zn^(2+)(aq)+2e^(-)hArrZn(s):E^(@)=-0.762V Cr^(3+)(aq)+3e^(-)hArrCr(s):E^(@)=-0.740V 2H^(+)(aq)+2e^(-)hArrH_(2)(g), E^(@)=0.000V Fe^(3+)(aq)+e^(-)hArrFe^(2+)(aq),E^(@)=0.770V Which is the stronget reducing agent?

The standard reduction potentials at 298K for the following half cells are given : ZN^(2+)(aq)+ 2e^(-)Zn(s) , E^(@) = - 0.762V Cr^(3+)(aq)+ 3e^(-) Cr(s) , E^(@) = - 0.740V 2H^(+) (aq)+2e^(-) H_(2)(g) , E^(@)= 0.000V Fe^(3+)(aq)+ e^(-) Fe^(2+)(aq) , E^(@) = 0.770V which is the strongest reducing agent ?

Electrode potential data are given below: Fe^(3+)(aq)+e^(-)rarrFe^(2+)(aq):E^(@)=+0.77V Al^(3+)+3e^(-)rarrAl(s):E^(@)=-1.66V Br_(2)(aq)+2e^(-)rarr2Br^(-)(aq):E^(@)=+1.08V , Based on the data, the reducing power of Fe^(2+) Al and Br^(-) will increase in the order

If the half cell reactions are given as (i) Fe^(2+)(aq)+2e^(-)rarrFe(s),E^(@)=0.44V (ii) 2H^(+)(aq)+ 1//2O_(2)(g)+2e^(-)rarrH_(2)O(l),E^(@)=+1.23V The E^(@) for the reaction.

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