Under which set of conditions is δgrxn for the reaction a(g) → b(g) most likely to be negative?

delta G = -ve.. This means the rxn is spontaneous

Explanation:

For spontaneous rxn

Delta H = - ve

Delta S = +ve

And no. Of moles at product side should be less than tha reactant side.

I wrote all i know.. Hope this helps you

This question is incomplete but the completed question is below

Under which set of conditions is ΔGrxn for the reaction A(g)→B(g) most likely to be negative?

Under which set of conditions is for the reaction most likely to be negative?

(a) PA=0.010 atm; PB=0.010 atm

(b) PA=0.010 atm; PB=10.0 atm

(c) PA=10.0 atm; PB =0.010 atm

(d) PA=10.0 atm; PB =10.0 atm

The correct option is (c)

Explanation:

The Gibb's free energy (ΔG) of the reaction will be negative when the reaction is spontaneous and a reaction is said to be spontaneous when more products are been formed.

When you consider the reaction provided in the question, the "g" in bracket means gas while A represent reactant(s) and B represents product(s)

When a reaction involves gases, an increase in pressure causes more products to be formed hence the pressure on the reactant side (PA) will most likely be more than the pressure on the product side (PB). The only option that has more pressure on the reactant side (PA = 10.0 atm) than on the product side (PB = 0.010 atm) is option c.

i have no clue hope you find the answer

wher is the rest of the question