The cell potential for the following cell `Pt |H_2(g)|H+ (aq)|| Cu^(2+) (0.01 M) Cu(s)`
is 0.576 V at 298 K. The pH of the solution is _____ (Nearest integer)
(Given: `E_(Cu^(2+//Cu))^@=` 0.34 V and `(2.303 RT)/F` = 0.06 V)

For the electrochemical cell shown below Pt|H_2(p=1atm)|H^+(aq.,xM)||Cu^(2+)(aq.,1.0M)|Cu(s) The potentialis 0.49 V at 298 K. The pH of the solution is closest to:[Given, standard reduction potential, E^@ for Cu^(2+)//Cu is 0.34 V. Gas constant, R is 8.31 JK^-1mol^-1 Faraday constant, F is 9.65xx10^4JV^-1mol^-1 ]

The standard e.m.f. for the cell reaction. 2Cu^(+)(aq)rarrCu(s)+Cu^(2+)(aq) is +0.36 V at 298K. The equilibrium constant of the reaction is

The cell potential for the cell Ni|Ni^(2+)(1M)||Cu^(2+)(1M)|Cu is 0.59 V and E(Cu^(2+)|Cu) = +0.34 V . What is the standard electrode potential of Ni^(2+)|Ni electrode?

For the cell Cu (s) | Cu ^(2+) (aq) (0.1 M) || Ag ^(+) (aq) (0.01 M) | Ag (s) the cell potential E _(1) = 0.3095 V For the cell Cu (s) | Cu ^(+2) (aq) (0.01 M) || Ag ^(+) (aq)( 0. 001 M) | Ag (s) the cell potential = _______ xx 10 ^(-2) V. (Round off the Nearest Integer). [Use : (2.303 RT)/(F) =0.059 ]

For the disproportionation reaction 2Cu^(+)(aq)hArrCu(s)+Cu^(2+)(aq) at K, In K (where K is the equilibrium constant) is ________ xx10^(–1) . Given : ( E_(Cu^(2+)//Cu^+)^@ = 0.16V and E_(Cu^(+)//Cu)^@ = 0.52V)

Which of the following statements is correct? If E_(Cu^(2+)|Cu)^(@)=0.34V "and"E_(H^+|H_2)^(@)=-0.0V

The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

What is the cell potential for following cell Zn(s)//Zn^(2+)(0.04M||Cu^(2+)(0.02M)//Cu(s) Given E_(Zn//Zn^(2+))^@ = -0.76V & E_(Cu//Cu^(2+))^@ = 0.34V