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During volcanic eruptions, hydrogen sulfide gas is given off and oxidised by air according to the following chemical equation: 2 H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) Calculate the standard enthalpy change for the reaction above, given: 3S(s) + 2H2O(g) → 2H2S(g) + SO2(g) ΔHP = 162.9 kJ mol−1 S(s) + O2(g) → SO2(g) ΔH = −306.5 kJ mol−1

During volcanic eruptions, hydrogen sulfide gas is given off and oxidised by air according to the following chemical equation: 2 H2S(g) + 3O2(g) → 2SO2(g) + 2H2O(g) Calculate the standard enthalpy change for the reaction above, given: 3S(s) + 2H2O(g) → 2H2S(g) + SO2(g) ΔHP = 162.9 kJ mol−1 S(s) + O2(g) → SO2(g) ΔH = −306.5 kJ mol−1

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During volcanic eruptions, hydrogen sulfide gas is given off and oxidised by air according to the following chemical equation:
2 H 2 S ( g ) + 3 O 2 ( g ) → 2 S O 2 ( g ) + 2 H 2 O ( g )
Calculate the standard enthalpy change for the reaction above, given:
3 S ( s ) + 2 H 2 O ( g ) → 2 H 2 S ( g ) + S O 2 ( g ) Δ H P = 162.9 k J m o l − 1 S ( s ) + O 2 ( g ) → S O 2 ( g ) Δ H = − 306.5 k J m o l − 1

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