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If for the half reactions Cu^(2+)+e^- ...

If for the half reactions
`Cu^(2+)+e^- to Cu^+" "E^0=0.15V`
`Cu^(2+)+2e^- to Cu" "E^0=0.34V`
Calculate `E^0` of the half cell reaction
`Cu^+ +e^- to Cu`
also predict whether `Cu^+` undergoes also predict whether `Cu^+` undergoes disproportionation or not

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The correct Answer is:
A, C, D
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E^@ values for the half cell reactions are given below : Cu^(2+) + e^(-) to Cu^(+) , E^@ =0.15 V Cu^(2+) + 2e^(-) to Cu, E^@ =0.34 V What will be the E^@ of the half-cell : Cu^(+) + e^(-) to Cu ?

If for the half cell reaction E^(@) value are given Cu^(2+)+e^(-)rarrCu^(+),E^(@)=0.15V Cu^(2+)+2e^(-)rarrCu^(+),E^(@)=0.34V calculate E^(@) of the half cell reaction Cu^(+)+e^(-)rarrCu

Given: (i) Cu^(2+)+2e^(-) rarr Cu, E^(@) = 0.337 V (ii) Cu^(2+)+e^(-) rarr Cu^(+), E^(@) = 0.153 V Electrode potential, E^(@) for the reaction, Cu^(+)+e^(-) rarr Cu , will be

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

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu

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