In an electrochemical cell the overall reaction is `Cd+Cu^(2+)(a=1)rarrCd^(2+)(a=1)+Cu`.
If `E^(0)` `Cd^(2+)|Cd=-0.403V` and `E^(0)` `Cu^(2+)|Cu=0.337V` at `298K`. Calculate the cell emf.

The following electrochemical cell is set up at 298 K: Zn//Zn^(2+) (aq) (1 M) || Cu^(2+) (aq) (1 M)//Cu Given: E^(@)Zn^(2+)//Zn =-0.761 V, E^(@) Cu^(2+)//Cu=+0.339 V (1) Write the cell reaction. (2) Calculate the emf and free energy change at 298 K

Consider the cell reaction : Mg(s)+Cu^(2+)(aq) rarr Cu(s) +Mg^(2+)(aq) If E^(c-)._(Mg^(2+)|Mg(s)) and E^(c-)._(Cu^(2+)|Cu(s)) are -2.37 and 0.34V , respectively. E^(c-)._(cell) is

E^(@) of Fe^(2 +) //Fe = - 0.44 V, E^(@) of Cu //Cu^(2+) = -0.34 V . Then in the cell

What is DeltaG^(@) for the following reaction Cu^(+2)(aq)+2Ag(s)rarrCu(s)+2Ag E_(Cu^(+2)//Cu)^(@)=0.34V E_(Ag^(+)//Ag)^(@)=0.8V

Calculate the emf of the given cell: Cu/ Cu^(2+)(0.01M) ∣∣ Cu^(2+) (0.001M)∣Cu is ( E^(@)Cu^(2+) /Cu=+0.34V)

Calculate E_("cell") at 25^(@)C for the reaction : Zn+Cu^(2+) (0.20M) to Zn^(2+) (0.50M)+Cu Given E^(Theta) (Zn^(2+)//Zn)= -0.76V, E^(Theta)(Cu^(2+)//Cu)=0.34V .

Given that standard potential for the following half - cell reaction at 298 K, Cu^(+)(aq)+e^(-)rarr Cu(s), E^(@)=0.52V Cu^(2+)(aq)+e^(-)rarrCu^(+)(aq), E^(@)=0.16V Calculate the DeltaG^(@)(kJ) for the eaction, [2Cu^(+)(aq)rarr Cu(s)+Cu^(2+)]

Calculate DeltaG^(@) for the reaction : Cu^(2+)(aq) +Fe(s) hArr Fe^(2+)(aq) +Cu(s) . Given that E^(@)Cu^(2+)//Cu = 0.34 V , E_(Fe^(+2)//Fe)^(@) =- 0.44 V

Calculate the e.m.f. of the cell Zn//Zn^(2+) (0.1M) "||" Cu^(2+) (0.01M) "|"Cu E_(Zn^(2+)//Zn)^(Theta)= -0.76 " V and "E_(Cu^(2+)//Cu)^(Theta)=0.34V

The e.m.f. ( E^(0) )of the following cells are Ag| Ag^(+)(1M) | | Cu^(2+)(1M) | Cu, E^(0) = -0.46V , Zn|Zn^(2+)(1M)| | Cu^(2+)(1M) | Cu : E^(0) = +1.10V Calculate the e.m.f. of the cell Zn | Zn^(2+)(1M) | | Ag^(+)(1M) | Ag