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)+h2o(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