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E^(0) for the reaction Fe + Zn^(2+) to ...

`E^(0)` for the reaction `Fe + Zn^(2+) to Zn + Fe^(2+)` is -0.35 V . The given cell reaction is

A

feasible

B

not feasible

C

explosive

D

slow

Text Solution

Verified by Experts

The correct Answer is:
B
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The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The E^@ for the reaction 2Cu^(+) to Cu^(2+) + Cu is :

The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The decrease in free energy during the cell reaction in Zn | Zn^(2+) (1M)||Cu^(2+)(1M)|Cu , when its changes to 1M(Zn^(+2)) and 0.1M(Cu^(+2)) is .........

The E^(@) values for the changes given below are measured against NHE at 27^(@) C Cu^(2+) + e to Cu^(+) , E^(@) = + 0.15 V , Cu^(+) + e to Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e to Zn , E^(@) = - 0.76 V . The temperature coefficient of emf a cell designed as Zn|Zn^(2+) || Cu^(2+) || Cu is - 1.4 xx 10^(-4)v per degree . For a cell reaction in equilibrium DeltaG= 0 and DeltaG^(@) = -2.303 RT log K_(c) . The heat of reaction and entropy changes during the reaction are related by DeltaG = DeltaH - TDeltaS . The equilibrium constant constant for the reaction : Zn + Cu^(2+) iff Zn^(2+) + Cu is

AAKASH SERIES-ELECTROCHEMISTRY -Exercise -2 (Nernst equation and EMF)
  1. EMF of a cell in terms of reduction potential of its left and right el...

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  2. E^(0) for the half cell Zn^(2+) // Zn is - 0.76 V . Emf of the cell ...

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  3. If the standard electrode protential of Cu^(2+)// Cu electrode is 0.34...

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  4. The potential of hydrogen electrode is -118 mV . The H^(+) concentrati...

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  5. The standard potential (E^(0)) for the half reaction are as Zn to Zn^...

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  6. E^(0) for F2 + 2e^(-) to 2F^(-) is 2.8 V , E^(0) for 1//2 F2 + e^(-) ...

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  7. Consider the following E^(0) values E(Fe^(3+) // Fe^(2+))^(0) = + 0.77...

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  8. E^(0) for the reaction Fe + Zn^(2+) to Zn + Fe^(2+) is -0.35 V . The ...

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  9. E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V ...

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  10. The EMF of the cell Ni//Ni^(2+)(0.01)// // Cl^(-)(0.01M)//Cl(2), pt i...

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  11. The standard electrode potential of the htwo half cells are given bel...

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  12. Aluminium displaces hydrogen from dilute HCl whereas silver does not. ...

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  13. A cell constructed by coupling a standard copper electrode and a stand...

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  14. The solution of nickel sulphate in which nickel rod is dipped is dilut...

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  15. The standard reduction potentials for the two half-cell reactions are ...

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  16. Normal aluminium electrode coupled with normal hydrogen electrode give...

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  17. The standard EMF for the cell reaction , Zn + Cu^(2+) to Cu + Zn^(2+) ...

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  18. At a certain temperature and at infinite dilution, the equivalent cond...

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  19. The emf of the following three galvanic cells are respresented by E(1)...

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