Using the Standard Entropy Values:
H₂(g), S° = +130 $\rarr$ 2 HI(g)
A)-40

Using the standard entropy values:
H₂(g) , S° = +130.6 J mol^-1 K^-1
I₂(s) , S° = +116.12 J mol^-1 K^-1
HI(g) , S° = +206.0 J mol^-1 K^-1
Calculate the standard entropy change, S°, for the reaction:H₂(g) + I₂(s) $\rarr$ 2 HI(g)

A) -40.8 J mol^-1 K^-1
B) +40.8 J mol^-1 K^-1
C) -165.3 J mol^-1 K^-1
D) +165.3 J mol^-1 K^-1
E) +206.0 J mol^-1 K^-1