[thermodynamics]

∆h_rxn = -670kj

45.8 g

Step-by-step explanation:

M_r: 34.08

         2H₂S + SO₂ ⇌ 3S + 2H₂O ; ΔH°r =  -670 kJ

1. Calculate the moles of H₂S

Treat the heat as if it were a product in the equation. Then use the molar ratio (2 mol H₂S/670 kJ) in the usual way.

Moles of H₂S = 450 kJ × 2 mol H₂S/670 kJ = 1.343 mol H₂S

2. Calculate the mass of H₂S

Mass of H₂S = 1.343 mol H₂S × (34.08 g H₂S/1 mol H₂S) = 45.8 g H₂S

You need 45.8 g of H₂S to produce 450 kJ of energy.

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