7. Energy, Rate and Equilibrium

Calculate the ∆H_rxn for the following thermochemical equation:

S (s) + $\frac{3}{2}$ O₂ (g) → SO₃ (s) ΔH_rxn = ?

When given the following:

2 S (s) + 3 O₂ (g) → 2 SO₃ (s) ΔH_rxn = −296.8 kJ

Calculate the ∆H_rxn for

$S\left(s\right)+\frac{3}{2}{O}_2\left(g\right)⟶S{O}_3\left(g\right);\Delta H{°}_{rxn}=?$

Given the following set of reactions:

$\frac{1}{2}S\left(s\right)+\frac{1}{2}{O}_2\left(g\right)⟶\frac{1}{2}S{O}_2\left(g\right);\Delta H°=-296.8kJ$

$2S{O}_3\left(g\right)⟶2S{O}_2\left(g\right)+O_2\left(g\right);\Delta H°=198.4kJ$

Calculate the ∆H_rxn for

ClF (g) + F₂ (g) → ClF₃ (g) ΔH_rxn = ?

Given the following reactions:

Cl₂O (g) + F₂O (g) → 2 ClF (g) + O₂ (g) ΔH° = −167.4 kJ

4 ClF₃ (g) + 4 O₂ (g) → 2 Cl₂O (g) + 6 F₂O (g) ΔH° = 682.8 kJ

2 F₂ (g) + O₂ (g) → 2 F₂O (g) ΔH_rxn = −181.7 kJ