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Calculate the equilibrium constant for t...

Calculate the equilibrium constant for the reaction:
`Fe^(2+)+Ce^(4+)hArr Fe^(3+)+Ce^(3+)`
Given : `E_((Ce^(4+)|Ce^(3+)))^(@)=1.44V, e_((Fe^(3+)|Fe^(3+)))^(@)=0.68V`

Text Solution

Verified by Experts

The half - cell reactions are as follows :
`{:("At anode: "Fe^(2+)(aq)" "rarr" "Fe^(3+)(aq)+e, E^(@)=-0.68V),("At cathode: "Ce^(4+)(aq)+e" "rarr" "Ce^(3+)(aq), E^(@)=1.44V),(bar("Cell reaction: "Fe^(2+)(aq)+Ce^(4+)(aq)hArr Fe^(3+)(aq)+Ce^(3+)(aq),E_("cell")^(@)=+0.76V)):}`
We know, `E_("cell")^(@)=(0.059)/(n)logK_(eq)" or, "+0.76=(0.059)/(1)log K_(eq)`
`"or, "logK_(eq)=(0.76)/(0.059)=12.859" "therefore" "K_(eq)=7.227xx10^(12)`
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Determine the equilibrium constant for the reaction : Fe^(2+)(aq)+Ce^(4+)(aq)rarr Fe^(3+)(aq)+Ce^(3+)(aq) Givne : E_(Ce^(4+)|Ce^(3+))^(@)=1.44V & E_(Fe^(3+)|Fe^(2+))^(@)=0.77V .

Find the equilibrium constant for the reaction: Cu^(2+)+In^(2+)hArr Cu^(+)+In^(3+) Given : E_(Cu^(2+)|Cu^(+))^(@)=0.15V, E_(In^(2+)|In^(+))^(@)=-0.4V, E_(In^(3+)|In^(+))^(@)=-0.42V

What will be the standard electrode potential for the change, Fe^(3+)(aq)+e rarr Fe^(2+)(aq). Given : E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Fe^(2+)|Fe)^(@)=-0.439V

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It the reaction, 2Ag(s)+Fe^(2+)(aq)rarr2Ag^(+)(aq)+Fe(s) possible? Given : E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V .

Calculate the equilibrium constant for the reaction : 2Fe^(3+)+3I^(-)hArr 2Fe^(2+)+I_(3)^(-) . Given: Standard reduction potential in acidic conditions is 0.78 V and 0.54 V, respectively, for Fe^(3+)|Fe^(2+) and I_(3)^(-)|I^(-) couples.

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (2) Fe+Sn^(2+)rarr Fe^(2+)+Sn Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

The following electrochemical cell has been set up: Pt(1)|Fe^(3+),Fe(a=1)||Ce^(4+), Ce^(3+)(a=1)|Pt(2) . If an ammeter is connected between two platinum electrodes, predict the direction of the flow of current. Will the current increase or decreases with time ? Given: E_((Fe^(3+)|Fe^(2+)))^(@)=0.77V and E_((Ce^(4+)|Ce^(3+)))^(@)=1.61V

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (1) Fe+CuSO_(4)rarr FeSO_(4)+Cu Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place: Fe%(2+)(aq)+Ag^(+)(aq)rarrFe^(3+)(aq)+Ag(s) Calculate the Delta_(r)G^(@) and equilibrium constant of the reaction also. (E_(Ag^(+)|Ag)^(@)=0.80V, E_(Fe^(3+)|Fe^(2+))^(@)=0.77V)

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