Calculate the reduction potential for the following half cell reaction at 298 K.
`Ag^(+)(aq)+e^(-)toAg(s)`
`"Given that" [Ag^(+)]=0.1 M and E^(@)=+0.80 V`

Calculate the reduction potentials for the following half cells: Ag|Ag^+ (10^-5 M),E_(Ag^+,Ag)^@=0.80V

Calculate the equilibrium constant of the following reaction aty 298K. Cu(s)+2Ag^+(aq) rarr Cu^(2+)(aq)2Ag(s)~ Given E_(cell)^Theta=0.46V

Calculate the standard reduction potentials of galvanic cells in which reaction are Fe^(2+) (aq) + Ag^(+) (aq) to Fe^(3+) (aq) + Ag (s) Given that E^(Theta) (Cr^(3+) //Cr) = -0.74 V , E^(Theta) (Cd^(2+) // Cd) = -0.40 V , E^(Theta) (Fe^(3+) // Fe^(2+)) = 0.77 V , E^(Theta) (Ag^(+) // Ag) = 0.80 V

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

Calculate emf and DeltaG for the following reaction at 298 K Mg(s)|Mg^(2+)(0.01 M)||Ag^(+)(0.0001 M)|Ag(s) Given E_((Mg^(2+)//Mg))^(@)=-2.37" V ", E_((Ag^(+)//Ag))^(@)=+0.80" V "

Calculate the emf for the following cell at 298 K. Cd//Cd^(2+)(0.1 M) || Ag^(+)(0.1 M)//Ag "Given"E_(Cd^(2+)//Cd)^(@)=-0.40" V ",E_(Ag^(+)//Ag)^(@)=0.80" V "

Calculate the E.M.F of the following cell at 298 K: Mg//Mg^(2+) (0.130 M)"||" Ag^(+) (1.0 xx 10^(-4)M) "|"Ag Given that E_((Mg^(2+)"|"Mg))^(Theta)= -2.37V, E_((Ag^(+)"|"Ag))^(@)=0.80V

Calculate the value of equilibrium constant for the reaction at 298 k. Cu(s) +2Ag^+(aq)rarrCu^(2+)(aq)+2Ag(s) E^@ (Ag2+/Ag) =0.80V and E^@( Cu2+/Cu ) =0.34V