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Whelan Whelan
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Posts: 3158
8 years ago
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.
Textbook 
Introductory Chemistry Essentials

Introductory Chemistry Essentials


Edition: 5th
Author:
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hbutler2hbutler2
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8 years ago
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