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(1) C(s, graphite)+ O2(g) → CO(g) AH =-393.5 kJ/mol (2) H2(g) + ¼O:(g) → H20(g) (3) C(s, graphite) + 2H2(g) → CH4(g) AH = -74.6 kJ/mol %3D AH =-241.8 kJ/mol %3D

(1) C(s, graphite)+ O2(g) → CO(g) AH =-393.5 kJ/mol (2) H2(g) + ¼O:(g) → H20(g) (3) C(s, graphite) + 2H2(g) → CH4(g) AH = -74.6 kJ/mol %3D AH =-241.8 kJ/mol %3D

Chemistry by OpenStax (2015-05-04)
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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4. Now use the enthalpy of formation values provided (values for equations 1-3 above) to calculate the enthalpy of combustion of methane. It should be the same as the number you came up with using Hess's Law.
Transcribed Image Text:4. Now use the enthalpy of formation values provided (values for equations 1-3 above) to calculate the enthalpy of combustion of methane. It should be the same as the number you came up with using Hess's Law.
Calorimetry can be used to measure enthalpy of a reaction and Hess's Law involves adding equations together to determine an unknown enthalpy of reaction. Another way to determine the enthalpy of a reaction is to use the standard enthalpy of formation of each component in a reaction. This is the energy absorbed or released when a compound is formed from elements in their standard states, the state at which the substance is most stable. For example, carbon dioxide, water, and methane can be formed according to the below reactions: (1) C(s, graphite) + O2(g) → CO2(g) AH¡ (2) H2(g) + ½O2(g) → H2O(g) (3) C(s, graphite) + 2H2(g) – CH4(g) AH, =-74.6 kJ/mol =-393.5 kJ/mol AH = -241.8 kJ/mol ntol form or most stable state, and, by definition,
Transcribed Image Text:Calorimetry can be used to measure enthalpy of a reaction and Hess's Law involves adding equations together to determine an unknown enthalpy of reaction. Another way to determine the enthalpy of a reaction is to use the standard enthalpy of formation of each component in a reaction. This is the energy absorbed or released when a compound is formed from elements in their standard states, the state at which the substance is most stable. For example, carbon dioxide, water, and methane can be formed according to the below reactions: (1) C(s, graphite) + O2(g) → CO2(g) AH¡ (2) H2(g) + ½O2(g) → H2O(g) (3) C(s, graphite) + 2H2(g) – CH4(g) AH, =-74.6 kJ/mol =-393.5 kJ/mol AH = -241.8 kJ/mol ntol form or most stable state, and, by definition,
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