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3 years ago Edited: 3 years ago, Anisha Aryal
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When 6.000 moles of H2(g) reacts with 3.000 mol of O2(g) to form 6.000 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 409.8 kJ of heat are released during this reaction, and PΔV is equal to -22.20 kJ, then A) ΔH° = +409.8 kJ and ΔE° = +432.0 kJ. B) ΔH° = +409.8 kJ and ΔE° = +387.6 kJ. C) ΔH° = -409.8 kJ and ΔE° = -387.6 kJ. D) ΔH° = -409.8 kJ and ΔE° = -432.0 kJ.
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