For the galvanic cell Mg(s)|Mg^(2+)(aq)|...

For the galvanic cell `Mg(s)|Mg^(2+)(aq)||Zn^(2+)(aq)|Zn(s)`,the standard free energy change is (`Given:E_((mg^(2+))/(mg))^@=`-2.36`V,E_((Zn^(2+))/(Zn))^@=`-0.76`V)`

`-1.6`F

`-3.2`F

`-4.8`F

`-F`

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The standard Gibbs free energy change (in joule) for the given cell reaction is Mg(s) + Ni^(2+) to Mg^(2+)(aq) + Ni(s) (Given: E_((mg)^(2+)/(mg))^@ = - 2.36 V , E_((NI)^(2+)/(NI))^@ = -0.25 V,

For the galvanic cell Zn(s)[Zn^2+ (aq)||Ag^+(aq) Ag(s)] , G° of the reaction in joule will be E°_ (Zn^(2+)) /( Zn )= - 0.76V , E°_( Ag_+)/(Ag )= 0.80 V

For the cell Zn(s)|Zn^(2+)(aq)||M^(x+)(aq)|M(s) different half cells and their standard electrode potentials are given below : If E^(@)Zn^(2+) |Zn = -0.76 V which cathode will given a maximum value of E^@ cell per electron transferred ?

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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 .

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At 25^(@)C temperature the cell potential of a given electrochemical cell is 1.92 V Mg(s)|Mg^(2+)(Aq)x M||Fe^(2+)(aq)0.01 M |Fe(s) Given E_(Mg//mg^(2+))(Aq)=2.37 v E_(Fe//Fe^(2+))^(@)(Aq)=0.45 V Find the value of x

For a standard cell Zn(s)|Zn^(2+)(1 M)||Cu^(2+)(1 M)|Cu(s) Write the electrode reaction and cell reaction. Also find the e.m.f. of cell if ? E_(Zn^(2+)|Zn)^(@)=-0.76" V", E_(Cu^(2+)|Cu)^(@)=+0.34" V" .

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