If an alkaline battery produces a cell potential of 1.46 v, what is the value of δgcell? the half-reactions in alkaline batteries are: $$zno (s) + h2 o (l) + 2e - zn (s) + 2oh - (aq)

The formula we're gonna use for this problem is written below:

ΔG° = nFE°

where

n is number of mol electrons displaced in the reaction

F is Faraday's constant = 96,500 C/mol e

E° is the standard emf

ΔG° = (2) (96,500) (1.46) = 281,780 Joules