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Author Question: The heat of combustion of methane is -50.38 kJ/mol. How many moles of methane must be burned to ... (Read 123 times)

sheilaspns

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on: Jul 8, 2021

Question 1

The final temperature when 150 mL of water at 90.0 °C is added to 100.0 mL of water at 30.0 °C is around ________.
◦ 90 °C
◦ 120 °C
◦ 30 °C
◦ 70 °C
◦ 25 °C

Question 2

The heat of combustion of methane is -50.38 kJ/mol. How many moles of methane must be burned to produce 137 kJ of heat?
◦ 6.90 mol
◦ 0.367 mol
◦ 2.72 mol
◦ 1.37 mol
◦ 0.272 mol
General Chemistry: Principles and Modern Applications ¦ Petrucci, Herring, Madura, Bissonnette ¦ 11th Edition
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Marked as best answer by sheilaspns on Jul 8, 2021

frogdreck123456

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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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sheilaspns

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

scottmt

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Reply 3 on: Yesterday
Great answer, keep it coming :)

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