The standard rectuion potentials for two half-cell reactions are given below
`Cd^(2+)(aq)+2e^(-)rarrCd(s),E^(@)=-0.40V`
`Ag^(+)(aq)+e^(-)rarrAg(s),E^(@)=0.80V`
The standard free energy change for the reaction
`2Ag^(+)(aq)+Cd(s)rarr2Ag(s)+Cd^(2+)(aq)` is given by

The standard reduction potentials for the two half-cell reactions are given below : Cd^(2+) (aq) + 2e^(-) to Cd(s) , E^(0) = -0.40 V " "Ag^(+)(aq) + e^(-) to Ag(s) , E^(0) = 0.80 V The standard free energy change for the reaction 2Ag_((aq))^(+) + Cd_((s)) + Cd_((aq))^(2+) is given by

The standard reduction potential for two reactions are given below AgCl(s)+e^(-)rarrAg(s)+Cl^(-)(aq) ,E^(@)=0.22V Ag^(+)(aq)+e^(-)rarrAg(s),E^(@)=0.80V The solubility product of AgCl under standard conditions of temperature is given by

The standard reduction potentials for two reactions are given below: AgCl(s)+barerarrAg(s)+Cl^(-)(aq) , E^@=0.22V and Ag^(+)(aq)+barerarrAg(s) , E^@=0.80V The K_(sp) of AgCl under standard conditions of temperature is given by

The reduction potential of the two half cell reaction (occurring in an electrochemical cell) are PbSO_(4)(s)+2e^(-)rarrPb(s)+SO_(4)^(2-)(aq)(E^(@)=-0.31V) Ag^(+)(aq)+e^(-)rarrAg(s)(E^(@)=0.80V) The feasible reaction will be

Use the standard reduction potentials: Sn^(2+)(aq) + 2e^(-) rightarrow Sn(s) E^(@) = -0.141V Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.800V To calcultate E^(@) for the reaction: Sn(s) + 2Ag^(+)(aq) rightarrow Sn^(2+)(aq) + 2Ag(s)

The standard reduction potentials for two reactions are given below: AgCl(s) + e^(-) to Ag(s) + Cl^(-) , E^@ = 0.22 V Ag^(+)(aq) e^(-) +e^(-) to Ag(s) , E^@ = 0.80V The solubility product of AgCl under standard conditions of temperature (298 K) is given by

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.