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Author Question: 8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 C and a ... (Read 122 times)

go.lag

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on: Jul 8, 2021
8.000 moles of H2(g) reacts with 4.000 mol of O2(g) to form 8.000 mol of H2O(l) at 25 °C and a constant pressure of 1.0133 bar. If 546.4 kJ of heat are released during this reaction, and PΔV is equal to -29.60 kJ, then:
◦ ΔH° = +546.4 kJ and ΔU = +576.06 kJ
◦ ΔH° = +546.4 kJ and ΔU = +516.8 kJ
◦ ΔH° = -546.4 kJ and ΔU = -516.8 kJ
◦ ΔH° = -546.4 kJ and ΔU = -576.0 kJ
General Chemistry: Principles and Modern Applications ¦ Petrucci, Herring, Madura, Bissonnette ¦ 11th Edition
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Marked as best answer by go.lag on Jul 8, 2021

sokh

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Reply #1 on: Jul 8, 2021
Lorsum iprem. Lorsus sur ipci. Lorsem sur iprem. Lorsum sur ipdi, lorsem sur ipci. Lorsum sur iprium, valum sur ipci et, vala sur ipci. Lorsem sur ipci, lorsa sur iprem. Valus sur ipdi. Lorsus sur iprium nunc, valem sur iprium. Valem sur ipdi. Lorsa sur iprium. Lorsum sur iprium. Valem sur ipdi. Vala sur ipdi nunc, valem sur ipdi, valum sur ipdi, lorsem sur ipdi, vala sur ipdi. Valem sur iprem nunc, lorsa sur iprium. Valum sur ipdi et, lorsus sur ipci. Valem sur iprem. Valem sur ipci. Lorsa sur iprium. Lorsem sur ipci, valus sur iprem. Lorsem sur iprem nunc, valus sur iprium.
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go.lag

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Reply 2 on: Jul 8, 2021
Gracias!

ryhom

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Reply 3 on: Yesterday
Excellent

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