Can we use a copper vessel to store 1 M `AgNO_(3)` solution?
Given
`E_(Cu^(2+)//Cu)^(Theta)=0.34V" "E_(Ag^(+)//Ag)^(Theta)=0.80`

Is it possible to store: (i) Copper sulphate solution in a zinc vessel? (ii) Copper sulphate solution in a silver vessel? (iii) Copper sulphate solution in a gold vessel? Given: E_(Cu^(2+)| Cu )^(0) = + 0.34 volt and E_(Ag^(2+)| Ag )^(0) = 0.80 volt and E_(Au^(2+)| Au )^(0) = +1.50 volt

Calculate the e.m.f. of the following cell at 298 K Co//Co^(2+)(0.1M)"||"Ag^(+) (0.1M)//Ag Given E_(Co^(2+)//Co)^(Theta)= -0.28 V, E_(Ag^(+)//Ag)^(Theta)=0.8V R = 8.31JK^(-1)"mol"^(-), F = 96500 coulombs.

What must be concentration of Ag^(+) in an aqueous solution containing Cu^(2+) =1.0 M so that bot the metals can be deposited on the cathode simultaneously. Given that E_(Cu//Cu^(2+))^(0)=0.34V and E_(Ag^(+)//Ag)^(0)=0.812V,T=298K

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

Consider a cell composed of two cells: (i). Cu(s)Cu^(2+)(aq) and (ii). Ag(s)|Ag^(+)(aq) (b). The cell potential when [Cu^(2+)]=2M and |Ag^(+)|=0.05M [Given: C_(Cu^(2+)//Cu)^(@)=+0.344V,E_(Ag^(+)//Ag)^(@)=+0.80V]

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

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

E_(Cu^(2+)//Cu)^(@) =0.43V E_(Cu^(+)//Cu)^(@)=0.55V E_(Cu^(2+)//Cu^(+))^(@) =

Why blue colour of CuSO_(4) solution gets discharged when zinc rod is dipped in it ? Given, E_(Cu^(+2)//Cu)^(@)=0.34 V and E_(Zn^(+2)//Zn)^(@)=-0.76V