ΔHrxn for the following reaction: 2CdS (s) + 3O₂ (g) → 2CdO (s) + 2SO₂ (g) will be -786.6 KJ
Write the balanced chemical equation for the reaction (1)
2H₂S (g) + O₂ (g) → 2S (s, rhombic) + 2H₂O (g) ΔH = -442.4 kJ
Write the balanced chemical equation for the reaction (2)
S (s, rhombic) + O₂ (g) → SO₂ (g) ΔH = -296.8 kJ
Write the balanced chemical equation for the reaction (3)
CdO (s) + H₂S (g) → CdS (s) + H₂O (g) ΔH = -124.7 kJ
To get reaction (4), multiply reaction (2) by 2
2S (s, rhombic) + 2O₂ (g) → 2SO₂ (g) ΔH = -593.6 kJ
To get reaction (5), reverse reaction (3) and multiply by 2
2CdS (s) + 2H₂O (g) → 2CdO (s) + 2H₂S (g) ΔH = 249.4 kJ
Finally add reaction (1), reaction (4), and reaction (5)
2CdS (s) + 3O₂ (g) → 2CdO (s) + 2SO₂ (g) ΔHrxn = -786.6 kJ
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