Home
Class 12
CHEMISTRY
For the reduction of NO(3)^(c-) ion in a...

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

A

`Fe` and `Au`

B

`Hg` and `Fe`

C

`V` and `Hg`

D

`Fe` and `V`

Text Solution

Verified by Experts

The correct Answer is:
b,c,d

`NO_(3)^(c-)+e^(-) rarr ?, E^(c-)._(red)=0.96V`
Compare the standard reduction potential of the given metals with that of `NO_(3)^(c-)` reduction.
`E^(c-)._(reduction)` for `NO_(3)^(c-)` is greater than `E^(c-)._(reduction)` of `(i),(ii),` and `(iv).`
So, `NO_(3)^(c-)` will be able to oxidize `Fe, Hg` and `V.`
So pairs are as in `(b),(c),` and `(d)`.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY|Exercise Archieves Single Correct|25 Videos
  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY|Exercise Archieves Fill In The Blanks|4 Videos
  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY|Exercise Archieves (Linked Comprehension )|13 Videos
  • D AND F BLOCK ELEMENTS

    CENGAGE CHEMISTRY|Exercise Archives Subjective|29 Videos
  • GENERAL PRINCIPLES AND PROCESS OF ISOLATION OF ELEMENTS

    CENGAGE CHEMISTRY|Exercise Archives (Subjective)|14 Videos

Similar Questions

Explore conceptually related problems

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) :

Given : Fe^(2+)(aq)+2e^(-) rarr Fe(s), " "E^(c-)=-0.44V Al^(3)+3e^(-) rarr Al(s)," "E^(c-)=-1.66V Br^(2+)+2e^(-)rarr 2Br^(c-)(aq)" "E^(c-)=-1.08V The decreasing order of reducing power is ……………………………….. .

Knowledge Check

  • 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)

    A
    V and Hg
    B
    Hg and Fe
    C
    Fe and Au
    D
    Fe and V
  • 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):

    A
    V and Hg
    B
    Hg and Fe
    C
    Fe and Au
    D
    Fe and V
  • For the reduction of NO_(3)^(-) ion in an aqueous solution, E^(0) is +0.96 V. Values of E^(0) for some metal ions ara given, below V^(2+) (aq) +2e^(-) to V E^(0)=-1.19V Fe^(3+) (aq)+3e^(-) to Fe E^(0)=-0.04 V Au^(3+) (aq) +3e^(-) to Au E^(0)=+1.40V Hg^(2+) (aq)+2e^(-) to Hg E^(0)=+0.86V The pair(s) of metals that is(are) oxidized by NO_(3)^(-) in aqueous solution is(are)

    A
    V and Hg
    B
    Hg and Fe
    C
    Fe and Au
    D
    Fe and V
  • Similar Questions

    Explore conceptually related problems

    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_((aq))^(2+)2e^(-)toV" "E^(0)=-1.19V Fe_((aq))^(3+)+3e^(-)toFe" "E^(@)=-0.04V Ag_((aq))^(3+)+3e^(-)toAu" "E^(0)=+1.40V Hg_((aq))^(2+)+2e^(-)toHg" "E^(o)=+0.86V The pair(s) of metals that is (areO oxidized by NO_(3)^(-) in aqueous solution is(are)

    Given standard E^(c-): Fe^(3+)+3e^(-)rarrFe," "E^(c-)=-0.036 Fe^(2+)+2e^(-)rarr Fe," "E^(c-)=-0.440V The E^(c-) of Fe^(3+)+e^(-) rarr Fe^(2+) is

    Half cell reactions for some electrodes are given below I. A + e^(-) rarr A^(-) , E^(@) = 0.96V II. B^(-) + e^(-) rarr B^(2-) , E^(@) = -0.12V III. C^(+) + e^(-) rarr C, E^(@) =+0.18V IV. D^(2+) + 2e^(-) rarr D, E^(@) = -1.12V Largest potential will be generated in which cell?

    Given : A^(2+)+2e^(-) rarr A(s)" "E^(c-)=0.08V B^(o+)+e^(-)rarr B(s)" "E^(c-)=-0.64V X_(2)(g)+2e^(-) rarr 2X^(c-)" "E^(c-)=1.03V Which of the following statements is // are correct ?

    Given, standard electrode potentials Fe^(2+) +2e^(-) rarr Fe, E^(@)=-0.440 V Fe^(3+)+3e^(-) rarr Fe, E^(@)=- 0.036 V The standarde potential (E^(@)) for Fe^(2+)+e^(-) rarr Fe^(2+) , is