What is the cell potential for following cell
`Zn(s)//Zn^(2+)(0.04M||Cu^(2+)(0.02M)//Cu(s)`
Given `E_(Zn//Zn^(2+))^@`= -0.76V & `E_(Cu//Cu^(2+))^@` = 0.34V

What is the cell potential of the following cell ? Zn(s)|Zn^(2+)(1.0M)||Pb^(2+)(1.0M)|Pb(s) Given : E_(Pb^(2+)//Pb)^(@)=-0.12" V and " E_(Zn^(2+)//Zn)^(@)=-0.76" V"

If the Zn^(2+) and Cu^(2+) concentrations are 0.1 M and 10^(-9) M respectively at 25^(@) C , the potential of the cell containing Zn//Zn^(2+) and Cu//Cu^(2+) electrodes is ___________. [Given E_(Zn//Zn^(2+))^(@)=+0.76, E_(Cu//Cu^(2+))^(@)=-0.34 V]

The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

Calculate the maximum work that can be obtained from the daniell call given below, Zn(s)|Zn^(2+)(aq)||Cu^(2+)(aq)|Cu(s) . Given that E_(Zn^(2+)//Zn)^(@)=-0.76V and E_(Cu^(2+)//Cu)^(@)=+0.34V .

Calculate E_(cell)^(0) of (at 298K) Zn(s)//ZnSO_(4)(aq)||CuSO_(4)(aq)//Cu(s) given that E_(Zn//Zn^(2+)(aq))^(0)=0.76V E_(Cu(s)//Cu^(2+)(aq))^(0)=-0.34V

Calculate E_("cell")^(0) of given electrochemical cell: Zn(s)+Cu^(2+) to Zn^(2+) (aq)+Cu(s) Given : E_(Zn^(2+)//Zn)^(0)=-0.76V E_(Cu^(2+)//Cu)^(0)=0.34V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V