Consider the following two reactions and the corresponding enthalpy changes: CH4(g) +2 O₂(g)-CO₂(g) +2 H₂O(1),AH₁ 2 CH4(g) + O₂(g) 2 CH3OH(1), H₂ Given that H₁ = −890 kJ, how much heat is released or absorbed in combustion of 1 mole of methane? 74.80 kJ released 149.6 kJ released 74.80 kJ absorbed 890 kJ absorbed 890 kJ released
Consider the following two reactions and the corresponding enthalpy changes: CH4(g) +2 O₂(g)-CO₂(g) +2 H₂O(1),AH₁ 2 CH4(g) + O₂(g) 2 CH3OH(1), H₂ Given that H₁ = −890 kJ, how much heat is released or absorbed in combustion of 1 mole of methane? 74.80 kJ released 149.6 kJ released 74.80 kJ absorbed 890 kJ absorbed 890 kJ released
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 49E: When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of...
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