The cell used in watch has the following cell reaction. Calculate `E^@` & `DeltaG^@` for it.
`Zn(s) + Ag_2O(s) + H_2O (l) rarr 2Zn^(2+) (aq) + 2Ag (s) + 2OH^- (aq)` Given `E^@_(Ag^+//Ag) = +0.80 V`, `E^@_(Zn^(2+)//Zn) = -0.76 V`

In the button cell, wiedly used in watches, the following reaction takes palce: Zn(s)+Ag_(2)O(s)+H_(2)O(l)rarr Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq) Determine E^(@) and DeltaG^(@) for the reaction. ["Given : "E_(Ag^(+)|Ag)^(@)=+080V, E_(Zn^(2+)|Zn)^(@)=-0.76V]

Consider the given reaction that occurs in a galvanic cell : Zn(s)+Ag_(2)O(s) +H_(2)O(l)rarr Zn^(2+)(aq)+2Ag(s)+2OH^(-)(aq) Write the cathode and the anode reactions.

Calculate the EMF of the electrochemical cell for which the following cell reaction is given below- Zx(S) + ni^(2_+)(aq) rarr Zn^(+2)(aq) + Ni(S) Given E_(zn^2//zn)^@ = - 0.76 V E_(Ni^(2+) // Nl) = - 0.25 V.

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (3) Zn+H_(2)SO_(4)rarr ZnSO_(4)+H_(2) Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Determine DeltaG^@ and the value of the equlibrium constant for the following reaction occurring in an electrochemical cell at 25^@C . Cu (s) + 2Ag^+ (aq) rarr Cu^(2+)(aq)+2Ag(s) Given that E_(Cu^(2+)//Cu)^@=0.34 V and E_(Ag^+//Ag)^@ =0.80V

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (2) Fe+Sn^(2+)rarr Fe^(2+)+Sn Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells : (1) Fe+CuSO_(4)rarr FeSO_(4)+Cu Given : E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V , E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V , E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V .

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V

The standard electrode potential of Daniell cell is 1.1V. Calculate the standard Gibbs energy for the reaction : Zn(s)+Cu^(2+)(aq)rarr Zn^(2+)(aq)+Cu(s)