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Author Question: HI has a normal boiling point of 35.4C, and its Hvap is 21.16 kJ/mol. Calculate the molar entropy of ... (Read 74 times)

Aimless0988

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on: Nov 5, 2023

Question 1

For the reaction HCONH2(g) NH3(g) + CO(g), Kc = 4.84 at 400 K.  If ΔH° for this reaction is 29 kJ/mol, find Kc at 500 K.
◦ 5.8
◦ 0.17
◦ 27
◦ 0.88
◦ 10.3

Question 2

HI has a normal boiling point of –35.4°C, and its ΔHvap is 21.16 kJ/mol.  Calculate the molar entropy of vaporization (ΔSvap).
◦ 598 J/K·mol
◦ 68.6 J/K·mol
◦ 75.2 J/K·mol
◦ 0.068 J/K·mol
◦ 89.0 J/K·mol
Chemistry ¦ Chang, Goldsby ¦ 11th Edition
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Marked as best answer by Aimless0988 on Nov 5, 2023

avelasquez

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Reply #1 on: Nov 5, 2023
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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Aimless0988

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Reply 2 on: Nov 5, 2023
Gracias!

dreamfighter72

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

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