Consider `Zn+Cu^(2+)rarrZn^(2+)+Cu`
If the standard emf is `E_("cell")=2.0V & F=96500 C`
Find `DeltaG^(@) (KJ "mol")`

The cell reaction Zn+Cu^(2+)rarrZn^(2+)+Cu , is best represented by-

For the cell reaction Zn(s) + Cu^(2+)(aq) rarr Cu(s) + Zn^(2+)(aq) E_("cell")^(@) = 1.10 V, DeltaG^(@) is :

The standard e.m.f. of the cell Zn+Cu^(2+)rarr Cu+Zn^(2+) is 1.10 V at 25^(@)C . The e.m.f. of the cell when 0.1 M Cu^(2+) and 0.1 M Zn^(2+) solutions are used will be

Consider the cell Zn|Zn^(2+) || Cu^(2+)|Cu. If the concentration of Zn and Cu ions are doubled, the emf of the cell.

Consider the cell Zn|Zn^(2+) || Cu^(2+)|Cu. If the concentration of Zn and Cu ions are doubled, the emf of the cell.

Consider the cell, Zn|Zn^(2+)(aq)(1.0M)||Cu^(2+)(aq)(1.0M)|Cu The standard reduction potentially are 0.350V for Cu^(2+)(aq)+2e^(-)rarrCu and -0.763V for Zn^(2+)(aq)+2e^(-)rarrZn (i) Write down the cell reaction (ii) Calculate the emf of the cell. (iii) Is the cell reaction spontaneous or not?

Consider the cell Zn|Zn^(2+) (aq) (1.0M) ||Cu^(2+) (aq) (1.0M) |Cu The standard reduction potentials are +0.35 V for 2e+ Cu^(2+) (aq) to Cu and -0.763V for 2e+Zn^(2+) (aq) to Zn Calculate the emf of the cell.