Which of the following relations represent correct relation between standard electrode potential and equilibrium constant ?
I. `logK = (nFE^(@))/(2303 RT)` II. `K = e^(-(nFE^(@))/(RT))`
III. `log K = (-nFE^(@))/(2303 RT)` IV. `log K = 0.4342 (nFE^(@))/(RT)`

Which of the following relation represents correct relation between standard electrode potential and equilibrium constant? I. logK = (nFE^(@))/(2.303RT) II. K = e^((nFE)/(RT)) III. log K = (-nFE^(@))/(2.303 RT) IV. log K = 0.4342 (-nFE^(@))/(RT) Choose the correct statement(s).

Which of the following relation represents correct relation between standard electrode potential and equilibrium constant? I. logK = (nFE^(@))/(2.303RT) II. K = e^((nFE)/(RT)) III. log K = (-nFE^(@))/(2.303 RT) IV. log K = 0.4342 (nFE^(@))/(RT) Choose the correct statement(s).

Which of the following is correct for Arrhenilus equation k=Ae^(-E_(a)//RT)

log K_p/K_c +log RT=0 is a relationship for the reaction :

log K_p/K_c +log RT=0 is a relationship for the reaction :

For which of the following gaseous reactions, the relationship log K_C/K_P+"log RT = 0" will bne correct ?

Derve the relation K_(p)=K_(c)(RT)^(Deltan_(g)) for a general chemical equilibrium reaction.

Derive the relation K_(p)=K_(c)(RT)^(Deltan_(g)) for a general chemical equilibrium reaction.