`E^(Theta)` of `Cu `is `+0.34 V `while that of `Zn `is `– 0.76 V`. Explain.

For the following cell, Zn(s) | ZnSO4(aq) || CuSO4(aq) | Cu(s) when the concentration of Zn2+ is 10 times the concentration of Cu2+, the expression for ΔG (in J mol–1) is [F is Faraday constant; R is gas constant; T is temperature; E° (cell) = 1.1V]

Find theta , 0 tan theta = 34.37 .

The e.m.f of the cell Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1xx10^-xM)|Cu is 2.651 V. The standard e.m.f of the cell is 2.71 V. the value of x is

The standard reduction potential for Cu^(2+)|Cu is +0.34V. Calculate the reduction potential at pH=14 for above couple. K_(sp) of Cu(OH)_2 is 1.0xx10^-19 .

A copper silver cell is set up. The copper ion concentration is 0.10 M. the concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. Given: E_(Ag^+|Ag)=+0.80V , E_(Cu^(2+)|Cu)=+0.34V

Aluminium displaces hydrogen fromacids, but copper does not. A galvanic cell prepared by combining Cu|Cu^(2+) and Al|Al^(3+) has an emf of 2.0V at 298K. If the potential of copper electrode is +0.34V, that of aluminium electrode is

Two metals A and B have reduction potentials values -0.76V and +0.34V respectively. Which of these will liberate H_2 from dil H_2SO_4 ?

The E°(M^2+/M) value for copper is positive (+0.34 V). What is the possible reason for this ?

The e.m.f of the cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag is 0.46V. The standard reductio potential of Ag^+|Ag is 0.80V. The standard reduction potential of Cu^(2+)|Cu is

E^(@) value for Cu^(2+)//Cu and Fe^(2+)//Fe are +0.34 V and -0.44 V respectively. Is the reaction Cu^(2+)+Fe to Cu+Fe^(3+) spontaneous or not ? Give reason also.