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E(cu)^(0)=0.34 and E(zn)^(0)=-0.76V. Cal...

`E_(cu)^(0)=0.34 and E_(zn)^(0)=-0.76V`. Calculate `E_("cell")^(0)`.

Text Solution

Verified by Experts

`E_("cell")^(0)=overset(oplus_(0))(E)-overset((-0)_(0))(E)`
`E_("cell")^(0)=E_("cell")^(0)-E_(Zn)^(0)=+0.34-(0.76)=+1.1V`
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E_(Cu)^(0)=+0.34V and E_(Ag)^(0)=+0.8V" calculate "E_(cell")^(0) .

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Knowledge Check

  • E_("red")^@ of different half cells are given below : E_(Cu^(2+)//Cu)^@ =0.34 V, E_(Zn^(+2)//Zn)^@ =-0.76 V,E_(Ag^+//Ag)^@ =0.80 V, E_(Mg^(+2)//Mg)^@ = -2.37 V . In which cell is Delta G^@ most negative ?

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    B
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    C
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