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Author Question: For the reaction H2(g) + 1/2 O2(g) H2O(g) rH = -241.8 kJ/mol, what mass of H2(g) is required to ... (Read 42 times)

debasdf

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on: Jul 8, 2021

Question 1

For a process at constant pressure, 49,600 calories of heat are released. This quantity of heat is equivalent to:
◦ 4.82 × 10-6 J
◦ 1.19 × 104 J
◦ 1.24 × 104 J
◦ 2.08 × 105 J

Question 2

For the reaction H2(g) + 1/2 O2(g) → H2O(g)  ΔrH° = -241.8 kJ/mol,
what mass of H2(g) is required to liberate 1.00 × 103 kJ of heat?
◦ 66.2 g
◦ 4.17 g
◦ 8.34 g
◦ 2.05 g
◦ 16.7 g
General Chemistry: Principles and Modern Applications ¦ Petrucci, Herring, Madura, Bissonnette ¦ 11th Edition
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Marked as best answer by debasdf on Jul 8, 2021

anoriega3

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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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debasdf

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Reply 2 on: Jul 8, 2021
Wow, this really help

Dinolord

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Reply 3 on: Yesterday
Thanks for the timely response, appreciate it

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