For the given concentration cell
` Cu(s)|Cu^(2+) (C_2 M) || Cu^(2+)(C_1 M) |Cu(s)`
Gibbs energy `triangle`G is negative if:

For the given concentration cell Cu(s)|Cu^(2+) (C_1 M) || Cu^(2+)(C_2 M) |Cu(s) Gibbs energy triangle G is negative if:

For the concentration cell Cu|Cu^(2+)(C_(1))||Cu^(2+)(C_(2))|Cu,DeltaG will be negative if

For the concentration cell Cu|Cu^(2+)(C_(1))||Cu^(2+)(C_(2))|Cu,DeltaG will be negative if Pt(Cl_(2)-P_(1))|HCl(0.1M)| Pt(Cl_(2)-P_(2)) the cell reaction is spontaneous if

Which of the following is the correct value of EMF of a following concentration cell? Cu|Cu^(2+)(0.01M)||Cu^(2+)(0.1M)|Cu at 25^(@)C

For the cell reaction , Cu^(2+)(aq)(C_2) +Zn(s) rarrZn^(2+)(aq)(C_1)+Cu(s) , the change in free energy (Delta G) at a given temperature is a function of :

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" .

Calculate the standard free energy change for the reaction : Zn(s)|Zn^(2+)(1 M)||Cu^(2+)(1 M)|Cu(s) Given E_(cell)^(@)=1.10" V " .

E^(@) for the electrochemical cell Zn(s)|Zn^(2+) 1 M (Aq.)||Cu^(2+) 1 M (aq.)|Cu(s) is 1.10 V at 25^(@)C . The equilibrium constant for the cell reaction, Zn(s) +Cu^(2+) (aq.) hArr Zn^(2+) (aq.)+Cu(s) Will be :

E^(@) for the electrochemical cell Zn(s) | Zn^(2+)1M (aq)|| Cu^(2+) 1M(aq)| Cu (s) is 1.10 V at 25^(@) C. The equilibrium constant for the cell reaction, Zn(s)+Cu^(2+) (aq.) rarr Zn^(2+) (aq.) + Cu(s) will be: