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CHEMISTRY · Subjective · A Level · Chemistry · Energetics · Energetics
Problem The enthalpy change Δ H x \Delta H_x Δ H x 2 SO 2 ( g ) + O 2 ( g ) → 2 SO 3 ( g ) 2\,\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\,\text{SO}_3(\text{g}) 2 SO 2 ( g ) + O 2 ( g ) → 2 SO 3 ( g ) 298 K 298\,\text{K} 298 K S ( s ) + O 2 ( g ) → SO 2 ( g ) \text{S}(\text{s}) + \text{O}_2(\text{g}) \rightarrow \text{SO}_2(\text{g}) S ( s ) + O 2 ( g ) → SO 2 ( g ) Δ H 1 = − 296.8 kJ \Delta H_1 = -296.8\,\text{kJ} Δ H 1 = − 296.8 kJ SO 3 ( g ) → SO 2 ( g ) + 1 2 O 2 ( g ) \text{SO}_3(\text{g}) \rightarrow \text{SO}_2(\text{g}) + \frac{1}{2}\,\text{O}_2(\text{g}) SO 3 ( g ) → SO 2 ( g ) + 2 1 O 2 ( g ) Δ H 2 = + 98.9 kJ \Delta H_2 = +98.9\,\text{kJ} Δ H 2 = + 98.9 kJ 2 S ( s ) + 3 O 2 ( g ) → 2 SO 3 ( g ) 2\,\text{S}(\text{s}) + 3\,\text{O}_2(\text{g}) \rightarrow 2\,\text{SO}_3(\text{g}) 2 S ( s ) + 3 O 2 ( g ) → 2 SO 3 ( g ) Δ H 3 = − 791.4 kJ \Delta H_3 = -791.4\,\text{kJ} Δ H 3 = − 791.4 kJ Δ H x \Delta H_x Δ H x Browse the problem library