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Following reactions occur at cathode dur...

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?

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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 ?

Au^(3+) + 3^(-) rightarrow Au(s) E^(@) = 1.50V Cu^(2+) + 2e^(-) rightarrow Cu(s) E^(@) = 0.34V According to the standard reduction potentials above, a substance that can oxidize only one of these metals must have an E^(@) value:

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)

Al^(3+)(aq) + 3e^(-) rightarrow Al(s) E^(@) = -1.66V Cu^(2+)(aq) + 2e^(-) rightarrow Cu(s) E^(@) = +0.34V What voltage is produced under standard conditions by combining the half-reactions witih these standard Electrode Potential?

Given the standard reduction potentials, which statement is correct? {:(Cu^(2)(aq) + 2e^(-) rightarrow Cu(s), E^(@) = 0.34V), (2H^(+)(aq) + 2e^(-) rightarrow H_(2)(g), E^(@)= 0.0V), (Cr^(3+)(aq) + 2e^(-) rightarrow Cr(s),E^(@) = -0.73V):}

A1^(3+) + 3e^(-) to Al(s) , E^(@) = -1.66V Cu^(2+)+ 2e^(-) rightarrow CU(s) , E^(@)=+0.34V What voltage is produced under standard conditions by combining the half reactions with these standard electrode potentials?

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