Calculate e.m.f. of the cell containing nickel and copper electrodes. Given that :
`E_(Ni^(2+)//Ni)^(@)=-0.25 V , E_(Cu^(2+)//Cu)^(@)=+0.34 V.`

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 .

Can 1M NiSO_(4) be stored in a veseel made up of copper? Given: E_(Ni^(2+)//Ni)^(@) = -1.20V and E_(Cu^(2+)//Cu)^(@) = 0.34V

Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal? Given that E_(Ni^(+2)//Ni)^(@)=0.25 " volt and "E_(Cu^(+2)//Cu)^(@)=+0.34" volt" .

Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal ? Given that E_(Ni^(+2)//Ni)^(@)=-0.25 volt and E_(Cu^(+2)//Cu)^(@) =+0.34 volt

If the Zn^(2+) and Cu^(2+) concentrations are 0.1 M and 10^(-9) M respectively at 25^(@) C , the potential of the cell containing Zn//Zn^(2+) and Cu//Cu^(2+) electrodes is ___________. [Given E_(Zn//Zn^(2+))^(@)=+0.76, E_(Cu//Cu^(2+))^(@)=-0.34 V]

Can a nicked spon be used to stir a solution of copper sulphate ? Support your answer with reaon. (Given : E_(Ni^(2+)//Ni)^(@)=-0.25" V", E_(Cu^(2+)//Cu)^(@)=0.34" V" )

Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal ? Given that E_(Ni^(-2)//Ni)=-0.25 volt and E_(Cu^(-2)//Cu)^(@) =+0.34 volt

Calculate the emf of the following cell: Cu(s)|Cu^(2+) (aq)||Ag^(+) (aq)| Ag(s) Given that, E_(Cu^(2+)//Cu)^(@)=0.34 V, E_(Ag//Ag^(+))^(@)=-0.80 V