Question

For the reaction :
X2O4 () ⟶2 XO2(g)
∆U = 2.1 k cal, ∆S = 20 cal K-1 at 300 K
Hence, ∆G is :

Answer 1

here you didn't mention that what is state of X2O4 ( ---)

step 1 :- find ∆H
∆H = ∆U + ∆ngRT
where ∆ng is The difference in gaseous molecule from product to reactant .

step 2 :-
use Gibbs free energy formula,
∆G = ∆H - T∆S
= ∆U + ∆ngRT - T∆S

then, you can find ∆G .

here I am not solving , becoz no mention what is the X2O4 { e.g gas , solid or liquid } without mentioned we can't solve this