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Following reactions occur at cathode dur...

Following reactions occur at cathode during electrolysis of aqueous silver chloride solution :
`Ag^(+)(aq)+e^(-) to Ag(s),E^(@)=+0.80" V"`
`H^(+)(aq)+e^(-) to 1//2 H_(2)(g), E^(@)=0.00" V"`
On the basis of standard reduction potential (`E^(@)` value), which reaction is feasible at cathode and why ?

Text Solution

Verified by Experts

Reaction with higher `E^(@)` value will be feasible since more then `E^(@)` value more will be the magnitudeof `-DeltaG^(@)(DeltaG^(@)=-nFE_(cell)^(@)`).
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Following reactions occur at cathode during the electrolysis of aqueous copper (II) chloride solution: CU_((aq))^(2+)+ 2e^(-)rightarrow Cu_(s), E^(@) = + 0.34V H_((aq))^(+) +e^(-) rightarrow (1)/(2)H_(2(s)), E^(@) = 0.00V On the basis of their standard reduction electrode potential (E^(@)) values, which reaction is feasible at the cathode and why?

Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.80V Co^(2+)(aq) + 2e(-) rightarrow Co(s) E^(@) = -0.28V Use the standard reduction potentials to determine the standard potential for the reaction: Co(s) + 2Ag^(+)(aq_) rightarrow Co^(2+)(aq) + 2Ag(s)

Consider a voltaic cell based on these half - cell reactions Ag^(+)(aq)+e^(-)rarrAg(s): E^(@)=+0.80V Cd^(+2)(aq)+2e^(-)rarrCd(s), E^(@)=-0.40V identify the anode and give the voltage of this cell under standard condition.

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