Home
Class 11
CHEMISTRY
Consider the following standard electrod...

Consider the following standard electrode potentials and calculate the eqillibrium constant at `25^(@)`C for the indicated disproportional reaction :
`3 Mn^(2+)(aq)toMn(s)+2Mn^(3+)(aq)`
`Mn^(3+)(aq)+e^(-)toMn^(2+)(aq), E^(@)=1.51 V`
`Mn^(2+)(aq)+2e^(-)toMn(s), E^(@)=-1.185 V``

A

`1.2xx10^(-43)`

B

`2.4xx10^(-73)`

C

`6.3xx10^(-92)`

D

`1.5xx10^(-62)`

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 1 (Q.1 To Q.30)|1 Videos

  • ELECTROCHEMISTRY

    NARENDRA AWASTHI|Exercise Level 1 (Q.91 To Q.120)|1 Videos

  • DILUTE SOLUTION

    NARENDRA AWASTHI|Exercise Level 3 - Match The Column|1 Videos

  • GASEOUS STATE

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|1 Videos

Similar Questions

Explore conceptually related problems

Calculate the equilibrium constant of the reaction : Cu_((s))+2Ag_((aq))^(+)to Cu_((aq))^(2+)+2Ag_((a)) E_((cell))^(Θ)=0.46V

The equilibrium constant for the following general reaction is 10^(@). Calculate E^(@) for the cell at 298 K. 2X_2(s) + 3Y^(2+)(aq) to 2X_(2)^(3+)(aq) + 3Y (s)

Write expression for the equilibrium constant, Ke for each of the following reactions. Fe_((aq))^(+3)++3OH_((aq))^(-) hArr Fe(OH)_(3(s))

Using the standard electrode potentials predict if the reaction between the following is feasible. (a) Fe^(3+) (aq) and I_(aq)^(-) (b) Ag_(aq)^(+) and Cu_(s)

Using the standard electrode potentials predict if the reaction between the following is feasible. a) Fe_((aq))^(3+) and I_((aq))^(-) b) Ag_((aq))^(+) and Cu_((s)

The standard electrode potential for the following reaction is + 1.33V.What is potential at pH=2.0? Cr_2O_7^(2-) (aq. 1M) + 14H^(+)(aq) + 6e^(-) to 2Cr^(3+) (aq. 1M0 + 7H_2O(l)

If the value of equilibrium constant (K_f) for the operation Zn_((aq))^(2+) + 4OH_((aq))^(-) iff Zn(OH)_(4(aq))^(2-) is 10^(10x) , then x is (Given : Zn_((aq))^(2+) + 2e^(-) to Zn_((s)) , E^(@)=-0.76 V , Zn(OH)_(4(aq))^(2-) + 2e^(-) to Zn_((s)) + 4OH_((aq))^(-) , E^(@) = - 1.36 V , 2.303 (RT)/(F) = 0.06 )

Using the standard electron potentials given in the Table 8.1, predict if the reaction between the following is feasible : (a) Fe^(3+) (aq) and I^(-) (aq) (b) Ag^(+)(aq) and Cu(s) (c) Fe^(3+) (aq) and Cu (s) (d) Ag(s) and Fe^(3+)(aq) (e) Br_(2) (aq) and Fe^(2+) (aq)

The standard emf of Deniell cell is 1.1 V. Calculate the standard Gibbs energy for the cell reactions: Zn_((s))+Cu_((aq))^(2+)to Zn _((aq))^(2+)+Cu_((s))

The standard reduction potentials at 298 K for the following half cell reactions are given below Zn^(2+) (aq) + 2e^(-) to Zn (s)-0.762 Cr^(3+) (aq) + 3e^(-) to Cr (s)-0.740 2H^(+) (aq) + 2e^(-) to H_(2) (g)-0.000 Fe^(3+) (aq) + e^(-) to Fe^(3+) (aq)-0.770 Which one is the strongest reducing agent?