Please help me with this

Question

Calculate delta G  at 298 K for the reaction

CS2(l)+3O2(g)⟶CO2(g)+2SO2(g)

based on these reactions.

C(s)+O2(g)⟶CO2(g)Δ𝐺∘=−397.28 kJ/mol

S(s)+O2(g)⟶SO2(g)Δ𝐺∘=−300.19 kJ/mol

C(s)+2S(s)⟶CS2(l)Δ𝐺∘=+62.37 kJ/mol

Delta G=KJ/mol?

Answer 1

Hess's Law:

CS₂(l) + 3O2(g)⟶CO₂(g) + 2SO₂(g) ... TARGET EQUATION

Given:

(1). C(s)+O2(g)⟶CO2(g ... Δ𝐺∘=−397.28 kJ/mol

(2). S(s)+O2(g)⟶SO2(g) ... Δ𝐺∘=−300.19 kJ/mol

(3). C(s)+2S(s)⟶CS2(l) ... Δ𝐺∘=+62.37 kJ/mol

Procedure:

reverse (3): CS2(l) ==> C(s) + 2S(s) ... ∆Gº = -62.37 kJ/mol

copy (1): C(s) + O2(g)⟶CO2(g) ... Δ𝐺∘ = −397.28 kJ/mol

copy (2) x 2: 2S(s) + 2O2(g) ==> 2SO2(g) ... ∆Gº = 2x-300.19 = -600.38 kJ/mol

Add all equations to get:

CS2(l) + C(s) + O2(g) + 2S(s) + 2O2(g) ==> C(s) + 2S(s) + CO2(g) + 2SO2(g)

Combine and cancel like terms to get ...

CS2(l) + 3O2(g) ==> CO2(g) + 2SO2(g) ... TARGET EQUATION

∆Gº = -62.37 + -397.28 + -600.38 = -1060 kJ/mol