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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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tennisnash2 tennisnash2
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8 years ago
When 0.250 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 177 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) ΔH = ?


Select one:


A. +1420 kJ

B. -708 kJ

C. -1420 kJ

D. +708 kJ
Post Merge: 8 years ago
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wrote...
#1
Educator
8 years ago
0.250 mol releases 177 kJ of heat

Thus, 2 moles would release (177 * 8 ) = 1416 kJ of heat.

Since, the heat is released, delta_H = negative.

Hence, answer is option C

-1420 kJ
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