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Cu^(+) + e rarr Cu, E^(@) = X(1) volt, ...

`Cu^(+) + e rarr Cu, E^(@) = X_(1)` volt,
`Cu^(2+) + 2e rarr Cu, E^(@) = X_(2)`X_(2) volt
For `Cu^(2+) + e rarr Cu^(+), E^(@)` will be :

A

`x_(1) -2x_(2)`

B

`x_(1)+2x_(2)`

C

`x_(1)-x_(2)`

D

`2x_(2)-x_(1)`

Text Solution

Verified by Experts

The correct Answer is:
D
`Cu^(+)+e^(-)rarr Cu Delta G_(1)= -F E^(@)= -FX_(1)`
`Cu^(2+)+2e^(-)rarr Cu Delta G_(2)= -2F E^(@)= -2 FX_(2)`
`Cu^(2+)+e^(-)rarr Cu^(+) Delta G_(3)= -2F E^(@)= -2 FX_(2)`
`Delta G_(3) = Delta G_(2)-Delta G_(1) -F E^(@)= -2 FX_(2)+FX_(1)`
`E^(@)=2X_(2)-X_(1)`
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Cu^(+) + e^(-) rightarrow Cu , E^(@) = x1volt , Cu^(2+) + 2e^(-) rightarrow Cu , E^(@) = x_(2) volt, then for Cu^(2+) + e^(-) rightarrow Cu^(+), E^(@) (volt) will be :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The E^(@) for the reaction : 2Cu^(+) rarr Cu^(2+) + Cu is:

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The E^(@) for Cu rarr Cu^(2+) + 2e is :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The E^(@) of Zn|Zn^(2+)||Cu^(2+)|Cu cell is :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The heat of reaction for the change Zn+underset(0.1 M)(Cu^(2+)) hArr underset(1M)(Zn^(2+))+Cu at 27^(@)C is :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . Change in entropy for the reaction : Zn+underset(0.1 M)(Cu^(2+)) hArrunderset(1M)(Zn^(2+))+Cu at 27^(@)C is :

The E^(@) values for the changes given below are measured againest NHE at 27^(@)C . Cu^(2+) + e rarr Cu^(+), E^(@) = + 0.15 V , Cu^(+) + e rarr Cu, E^(@) = + 0.50 V , Zn^(2+) + 2e rarr Zn, E^(@) = - 0.76 V The temperature coefficient of emf a cell designed as Zn"|"underset(1 M)(Zn^(2+))"||"underset(0.1 M)(Cu^(2+))"|"Cu is -1.4 xx 10^(-4)V per degree. For a cell reaction in equilibrium DeltaG = 0 and DeltaG^(@) = -2.303 RTlog_(10)K_(c) . The heat of reaction and entropy change during the reaction are are related by DeltaG = DeltaH - TDeltaS . The equilibrium constant for the reaction: Zn+Cu^(2+) hArr Zn^(2+)+Cu is:

Goven : (i) CU^(2+) + 2e^- rarr Cu, E^@ = 0.337 V (ii) Cu^(2+) +e^- rarr Cu^(+) , E^2=0.1 5 3 V .

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