In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(l) -> AH-890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.52 g of methane is combusted at constant pressure.
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(l) -> AH-890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.52 g of methane is combusted at constant pressure.
Chemistry: An Atoms First Approach
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ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
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Transcribed Image Text:QUESTION 1
In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:
CH4(g) + 2 O2(g)
CO2(g) + 2 H₂O(1) AH = -890.0 kJ
Calculate the value of q (kJ) in this exothermic reaction when 1.52 g of methane is combusted at constant pressure.
-84.6kJ
QUESTION 2
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