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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 c

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Posts: 3158
6 years ago
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.
Textbook

Introductory Chemistry Essentials

Edition: 5th
Author:
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hbutler2hbutler2
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6 years ago
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