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Author Question: When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical ... (Read 150 times)

karateprodigy

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on: Jul 8, 2021
When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written.

2 CH4(g) + 3 Cl2(g) → 2 CHCl3(l) + 3 H2(g) ΔrH° = ?

◦ -1420 kJ mol-1
◦ -708 kJ mol-1
◦ +708 kJ mol-1
◦ +1420 kJ mol-1
General Chemistry: Principles and Modern Applications ¦ Petrucci, Herring, Madura, Bissonnette ¦ 11th Edition
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Marked as best answer by karateprodigy on Jul 8, 2021

Sophiapenny

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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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karateprodigy

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

Dnite

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

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