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.`

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

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

Write cell reaction and calculate electrical work obtained from the following galvanic cell at standard condition . Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag [Given : E_(Mg^(2+)|Mg)^(0) = -2.36 volt and E_(Ag^(+)|Ag)^(0) = 0.80 volt.]

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

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 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 E_("cell")^(@) for the following reaction at 298K : 2Al(s)+3Cu^(2+)(0.01M)rarr 2Al^(3+)(0.01M)+3Cu(s) [GIven E_(cell)=1.98V ]

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 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 the cell in which the given reaction occurs : Mg(s)+2Ag^(+)(0.0001M)rarr Mg^(2+)(0.134M)+2Ag(s) Calculate its E_("cell") if E_("cell")^(@)=3.17V.