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.

Ag^(+)(aq)+e^(-)rarrAg(s) E^(@)=0.80V Cu^(2+)(aq)+2e^(-)rarrCu(s) E^(@)=0.34V Which expression gives the voltage for this cell if [Cu^(2+)]=1.00M and [Ag^(+)]=0.010M ?

Ag^(+)(aq)+e^(-)rarrAg(s) E^(@)=0.80V Cu^(2+)(aq)+2e^(-)rarrCu(s) E^(@)=0.34V Which increases immediately if the surface area of the silver electrode is increased?

Ag^(+)(aq)+e^(-)rarrAg(s) E^(@)=0.80V Cu^(2+)(aq)+2e^(-)rarrCu(s) E^(@)=0.34V What is the value for DeltaG^(@) when [Ag^(+)]=[Cu^(+)]=1.0M ?

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 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 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

Given the cell reactions MX_((s))+e^(-)rarrM_((s))+X_((aq))^(-),E^(@)=0.207V and M_((aq))^(+)+e^(-)rarrM_((s)),E^(@)=0.799V The solubility of MX_((s)) at 298K is