Consider the following reaction,
`Cu|Cu^(2+) (1M)||(Zn^(2+)(1 M)|Zn`
A cell represented above should have emf

Consider the following reaction, Zn(s)+Cu^(2+) (0.1 M) rarr Zn^(2+) (1 M)+Cu(s) above reaction, taking place in a cell, E_("cell")^(@) is 1.10 V. E_("cell") for the cell will be (2.303 (RT)/(F)=0.0591)

Consider the following reaction, Zn(s)+Cu^(2+) (0.1 M) rarr Zn^(2+) (1 M)+Cu(s) above reaction, taking place in a cell, E_("cell")^(@) is 1.10 V. E_("cell") for the cell will be (2.303 (RT)/(F)=0.0591)

Consider the reaction, Zn + Cu^(2+) rarr Zn^(2+) + Cu With reference to the above, which one of the following is the correct statement ?

The measured EMF at 298 K for the cell reaction, Zn(s) + Cu^(2+)(1.0 M) rarr Cu(s) + Zn^(2+)(0.1M) is 1.13 V. Calculate E^(@) for the cell reaction.

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.

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 Is the cell reaction spontaneous or not?

For the redox reaction Zn(s) + Cu^(2+) (0.1M) rarr Zn^(2+) (1M) + Cu(s) that takes place in a cell, E^(o)""_(cell) is 1.10 volt. E_(cell) for the cell will be: