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Title: When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C and a c Post by: Whelan on May 6, 2015 When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PΔV is equal to -74.00 kJ, then
A) ΔH° = +1366 kJ and ΔE° = +1440 kJ. B) ΔH° = +1366 kJ and ΔE° = +1292 kJ. C) ΔH° = -1366 kJ and ΔE° = -1292 kJ. D) ΔH° = -1366 kJ and ΔE° = -1440 kJ. Title: Re: When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C ... Post by: hbutler2 on May 24, 2015 Content hidden
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