Question

Relationship between equilibrium constant of the reaction and standard electrode potential of electrochemical cell in which that reaction takes place is ____________.

पर्याय

• `"E"_"cell"^0 = (2.303  "RT")/("nF") log "K"_"c"`

• `"E"_"cell"^0 = (2.303  "RT")/("F") log "K"_"c"`

• `"E"_"cell"^0 = (2.03  "RT")/("nF") log "K"_"c"`

• `"E"_"cell"^0 = (2.230  "RT")/("nF") log "K"_"c"`

Answer 1

Relationship between equilibrium constant of the reaction and standard electrode potential of electrochemical cell in which that reaction takes place is `underline("E"_"cell"^0 = (2.303  "RT")/("nF") log "K"_"c")`.

Explanation:

∆G⁰ = − 2.303 RT log K_c; ∆G⁰ = `-"nFE"_"cell"^0`

Equating, `"E"_"cell"^0 = (2.303  "RT")/"nF" log "K"_"c"`