Write the Nernst equation and emf of the following cell at 298K.
`Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M ) | H_(2) ( g) ( 1"bar") | Pt`.

Write the Nernst equation and emf of the following cells at 298K. (i) Sn(s) | Sn^(2+) ( 0.050M)|| H^(+) ( 0.020M)| H_(2) ( g, 1"bar") | Pt(s) (ii) Pt(s) | Br_(2) ( l ) | Br^(-)(0.010M) || H^(+) (0.030M) | H_(2)(g, 1"bar") | Pt (s)

Write the Nernst equation and emf of the following cell at 298 K. (i) Mg(s) |Mg^(2+) ( 0.001 M) || Cu^(2+) ( 0.0001M ) | Cu(s) (ii) Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M) | H_(2)(g) (1 "bar") | Pt(s) Given that, E_(Mg^(2+) //Mg)^(@) = - 2.36V , E_(Cu^(2+) Cu)^(@) = 0.34V, E_(Fe^(2+)Fe)^(@) = -0.44V

Calculate the emf of the following cell at 25^(@)C Fe|Fe^(@+) ( 0.001 M ) || H^(+) ( 0.01M ) || H_(2) ( g) ( 1 "bar" ) | Pt (s) E_((Fe^(@+) //Fe))^(@) = - 0.44 V , E_((H^(+) //H_(2)))^(@) = 0.00V

Write the Nernst equation to calculate the cell potential of Mg (s) | Mg^(2+) (aq) || Ag^(+) |Ag .

Calculate the EMF of following cell at 298K Fe(s) |Fe^(2+)(0.1M)| | Ag^(+)(0.1M)|Ag(s) Fe^(2+)|Fe = - 0.41V, Ag^(+)|Ag = +0.80V

Write the Nernst equation for the electrode reaction. M^(n+) ( aq) + n e^(-) rarr M(s) E = E^(@) - ( 2.303 RT )/( nF ) log""( [ M ] )/([ M ^(n+)])

Calculate the emf of the following cell. Zn(s)|Zn^(2+) (0.01M)|| Ag^+ (0.001M) | Ag(s) Given E_(Zn|Zn^(2+))^@ = 0.76V and E_(Ag|Ag^+)^@ = -0.80V

Calculate the emf of the cell in which the following reaction takes place, Ni(s) + 2Ag^(+) ( 0.002M) rarr Ni^(2+) ( 0.160M) + 2Ag(s) Given that E_("cell")^(@) = 1.05V

The potential of the following cell is 0.34 V at 25^(@)V . Calculate the standard reduction potential of the copper half-cell . Pt| H_(2) ( 1 atm) | H^(+) ( 1M) || Cu^(2+) ( 1M) | Cu