Write the Nernst equation for the above cell, if
`E^@(Zn^(2+)|Zn)=-0.76V, E^@(Cu^(@+)|Cu)=+0.34V`

Can a zinc spoon be used to stir a solution of copper sulphate? Support your answer with reason E_(Zn^(2+)|Zn)^@=-0.76V , E_(Cu^(2+)|Cu)^@=+0.34V

Derive Nernst equation for the following cell: NiNi^(2+)(0*2M)||Cu^(2+)(0*2M)|Cu .

A cell raction is n (s)| Sn_((0.50M))^(2+)//H_((0.020M))^(+)//H_(2)(g) . Calculate E_("cell") of a reaction and also write Nernst equation. Given: E^(@)(sin^(2+)|Sn)= -0.14V and E^(@)(H^(1+)|H)= 0.00V

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

Write Nernst equation and cell reaction of the following cell: Zn|Zn^(2+)||Cu^(2+)|Cu

Derive Nernst equation for the following cell: Cu|Cu^(2+)(0.1M)||Ag^(+)(0*1M)|Ag

Write the Nernst equation and emf of the following cells at 298 K: Mg(s)|Mg^(2+)(0.001M) || Cu^(2+)(0.0001 M)| Cu(s)

Calculate the EMF of the cell, containing nickel and copper electrodes. Given E^@(NI^(2+)|NI)=-0.25V and E^@(Cu^(2+)|Cu)=+0.34V .