The standard electrode potential `E^(@)` and its temperature coefficient `((dE^(@))/(dT))` for a cell are 2V and `-5xx10^(-4) Vk^(-1)` at 300K respectively . The cell reaction is ` Zn(s)+ Cu^(2) (aq)+ Cu(S)` .
The standard reaction enthalpy `Delta_(r) H^(@)` at 300 K `KJmol^(-1)` is :
`([use R = 8 JK^(-1)mol^(-1)` and `F = 96000Cmol^(-1)])`

The standard electrode potential E^(Theta) and its temperature coefficent ((dE^Theta)/(d T)) for a cell are 2V and -5xx10^(-4)VK^(-1) at 300 K respectively. The cell reaction is Zn(s)+Cu^(2+)(aq)to Zn^(2+)(aq) +Cu(s) . The standard reaction enthalpy (Delta_(t)H^(Theta)) at 300 K is 4.12 xx10^(x) J//"mol" . Numerical value of x is _________________ [Use R=8JK^(-1)mol^(-1) and F=96,000 C "mol"^(-1) ].

The standard electrode potential E^(Theta) and its temperature coefficent ((dE^Theta)/(d T)) for a cell are 2V and -5xx10^(-4)VK^(-1) at 300 K respectively. The cell reaction is Zn(s)+Cu^(2+)(aq)to Zn^(2+)(aq) +Cu(s) . The standard reaction enthalpy (Delta_(t)H^(Theta)) at 300 K is 4.12 xx10^(x) J//"mol" . Numerical value of x is _________________ [Use R=8JK^(-1)mol^(-1) and F=96,000 C "mol"^(-1) ].

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

The standard electrode potential (E^@) for Daniel cell is +1.1V. Calculate the Delta G^@ for the reaction. Zn(s)+Cu^(2+) (aq) to Zn^(2+) (aq)+Cu(s)

If the standard electrode potential for a cell is at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu^(2+) (aq) at 300 k is approximately : (R=8JK^(-1) mol^(-1) , F= 96000 mol^(-1))

If the standard electrode potential for a cell is 2V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu^(2+) (aq) at 300 k is approximately : (R=8JK^(-1) mol^(-1) , F= 96000 mol^(-1))

If the standed electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s)+Cu^(2+)(aq) hArrZn^(2+)(aq)+Cu(s) at 300 K is approximately (R=8JK^(-1)mol^(-1),F=96000Cmol^(-1))

If the standed electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s)+Cu^(2+)(aq) hArrZn^(2+)(aq)+Cu(s) at 300 K is approximately (R=8JK^(-1)mol^(-1),F=96000Cmol^(-1))

At 25^@C the EMF of the cell Zn, ZnSO_4"//"CuSO_4, Cu is 0.03V . The temperature coefficient of EMF is -1.4 xx 10^(-4) VK^(-1) . Calculate the enthalpy change of the cell reaction .