For an electrode reaction written as `M^(n+)+n e^(-)rarr M` , `E_(\"r
Channel: Doubtnut
Date: 16/02/2020

For an electrode reaction written as `M^(n+)+n e^(-)rarr M` , `E_(\"red\")=E_(\"red\")^(@)-(RT)/(nf)ln(1)/([M^(n+)])` `=E_(\"red\")^(@)-(0.059)/(n)\"llog\"(1)/([M^(n+)])` at 298 k For the cell reaction `aA+bB rarr xX+yY` `rArr E_(\"cell\")=E_(\"cell\")^(@)-(RT)/(nf)\"log\"([X]^(x)[Y]^(y))/([A]^(a)[B]^(b))` For pure solids, liquids or gases at lampt. molarconc = 1 Std. free energy change `Delta G^(@)=-nfE^(@)` where f - for faraday = 96,500 c, n = no. of `e^(-)` `Delta G=-2.303 RT log K_(c )` where `K_(c )` is equilibrium constant `K_(c )` can be calculated by using `E^(@)` of cell. The emf of the cell `Zn//zn^(2+)(0.01M)//Fe^(2+)(0.001M)//Fe` at 298 K is `0.2905`. The value of equilibrium constant for cell reaction si