The enthalpy of the chemical reaction: ΔH rxn = -1075 kJ/mol
Further explanation
Based on the principle of Hess's Law, the change in enthalpy of a reaction will be the same even though it is through several stages or ways
Reaction
CS₂ (l) + 3O₂(g) ---> CO₂(g) + 2SO₂ (g)
1. C(s)+O₂(g)⇒CO₂(g) ΔH=-393.5 kJ/mol
2. S(s)+O₂(g)⇒SO₂(g) ΔH=-296.8 kJ/mol x 2
2S(s)+2O₂(g)⇒2SO₂(g) ΔH=-593.6 kJ/mol
3. C(s)+2S(s)⇒CS₂(l) ΔH=+87.9 kJ/mol
Reverse
CS₂(l)⇒C(s)+2S(s) ΔH=-87.9 kJ/mol
Add all and remove the same compound on different sides
C(s)+O₂(g)⇒CO₂(g) ΔH=-393.5 kJ/mol
2S(s)+2O₂(g)⇒2SO₂(g) ΔH=-593.6 kJ/mol
CS₂(l)⇒C(s)+2S(s) ΔH=-87.9 kJ/mol
---------------------------------------------------------------+
CS₂ (l) + 3O₂(g) ---> CO₂(g) + 2SO₂ (g) ΔH=-1075 kJ/mol
