Calculate the E.M.F. for the cell given below `Mg(S)|Mg^(2+)(0.001)(M)||Cu^(2+)(0.01M)|Cu(S)` given `E_(Mg^(2+)//Mg)^@` =-2.36V. `E_(Cu^(2+)//Mg)^@`=+0.34V

Calculate the E.M.F. for the cell given below and identify the cathod and anode. Mg (S) | Mg^(2+) (0.001M) || CU^(2+) (0.01M) | Cu(S) E_(Mg^(2+)//Mg) = - 2.36 V and E_(Cu^(2+)//Cu) = + 0.34 V.

Write the Nernst equation & EMF of the cells at 298 K : Mg(s)|Mg^(2+)(0.001M)||Cu^(2+)(0.0001M)|Cu(s)

For the given cell, Mg|Mg^(2+)||Cu^(2+)|Cu -

Calculate the potential of the following cell at 298 K Zn//Zn^(2+)(a=0.1)//Cu^(2+)(a=0.01)//Cu E_(Zn^(2+)//Zn)^(@)=-0.762V E_(Cu^(2+)//Cu)^(@)=+0.337V Compare the free energy change for this cell with the free enegy of the cell in the standard state.

Determine the maximum amount of work that can be derived from the cell, Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu. Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V

Calculate E_("cell")^(@) of the cell Mg|Mg^(2+)||Cu^(+)|Cu Given : E_(Mg^(2+)|Mg)^(@)=-2.37V and E_(Cu^(+)|Cu)^(@)=+0.15V .

Calculate the electrical work (at standard state) obtained from galvanic cell : Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag Given : E_(Mg^(2+)|Mg)^(@)=-2.36V and E_(Ag^(2+)|Ag)^(@)=+0.80V

Calculate DeltaG^@ in kJmol^(2+) and equilibrium constant for the following cell reaction: Zn(s)+Cu^(2+)(aq)harrCu(s)+Zn^(2+)(aq) [Give: E_(Zn^(2+)//Zn)^@=-0.76 V, E_(Cu^(2+)//Cu)^@=+0.34V,F=96500 C mol^(-1)]

Calculate the emf of the following call at 298 K : 2Cr(s)+3Fe^(2+)(0.1M)rarr2Cr^(3+)(0.01M)+3Fe(s) ["Given : "E_((Cr^(3+)|Cr))^(@)=-0.74V, E_((Fe^(2+)|Fe))^(@)=-0.44V]

Calculate the emf and write the chemical reaction for the cell constructed with AI|AI^(3+)(0.01 M) and NI|Ni^(2+)(0.2 M) , E_(Ni^(2+)//Ni)^@ =-0.25V E_(AI^(3+)//AI)^@ =-1.66V