Given that
`E_(Cu^(2+)|Cu)=0.34V`
`E_(Mn^(+2)|Mn)^(@)=-1.18V`
Then the emf of the cell at `25^(@)C` is
`Mn|Mn^(2+)(0.1M)||Cu^(2+)(0.1M)|Cu`

Given that E_(cu^(+2)//cu)^(@)=+0.34 V E_(Mg^(+2)//Mg)^(@)=-2.37V which of the following correct

Given that E_(Cu^(2+)//Cu)^(0)=0.337 and E_(Cu^(+)//Cu^(2+))^(0)=-0.153V . then calculate E_(Cu^(+)//Cu)^(0)

If E_(Cu^(2+)|Cu)^(@) = 0.34V and E_(Cu^(2+)|Cu^(+))^(@)= 0.15 V then the value for disproportion for Cu^(+) is :

The e.m.f. ( E^(0) )of the following cells are Ag| Ag^(+)(1M) | | Cu^(2+)(1M) | Cu, E^(0) = -0.46V , Zn|Zn^(2+)(1M)| | Cu^(2+)(1M) | Cu : E^(0) = +1.10V Calculate the e.m.f. of the cell Zn | Zn^(2+)(1M) | | Ag^(+)(1M) | Ag

A graph is plotted between E_(cell) and log .([Zn^(2+)])/([Cu^(2+)]) . The curve is linear with intercept on E_(cell) axis equals to 1.10V . Calculate E_(cell) for the cell. Zn(s)||Zn^(2+)(0.1M)||Cu^(2+)(0.01M)|Cu

Given that (at T = 298 K) Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V Then E_(cell) for, Zn | Zn^(2+)(0.1M) || Ag^(+)(0.1M) | Ag at 298 K will be:

If E_((Mg)/(Mg^2+))^0 = +2.37 and E_((Cu)/(Cu^2+))^0 = -0.34 V then standard EMF of the cell, (Mg)/(Mg^(2+))/(Cu^(2+))/(Cu) is

Write the nearest equation and calculate the e.m.f. of the following cell at 298 K Cu(s)|Cu^(2+)(0.130M)||Ag^(+)(1.00xx10^(-4)M)|Ag(s) Given :E_(Cu^(2+)//Cu)^(@)=0.34V and E_(Ag^(+)//Ag)^(@)=+0.80V

(a) A cell is prepared by dipping a zinc rod in 1M zinc sulphate solution and a silver electrode in 1M silver nitrate solution. The standard electrode potential given : E^(@)Zn_(2+1//Zn) = -0.76V, E^(@)A_(g+//)A_(g) = +0.80V What is the effect of increase in concentration of Zn^(2+) " on the " E_(cell) ? (b) Write the products of electrolysis of aqueous solution of NaCI with platinum electrodes. (c) Calculate e.m.f. of the following cell at 298 K: "Ni(s)"//"Ni"^(2+)(0.01M)////"Cu"^(2+)(0.1M)//"Cu(s)" ["Given"E_(Ni2+//Ni)^(@) = -0.025 V E_(Cu2+//Cu)^(@) = +0.34V] Write the overall cell reaction.

Given : E^(@) (Cu^(2+//Cu) = 0.337V and E^(@) (Sn^(2+//Sn) = -0.136V . Which of the following statements is correct?