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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) - (2) H2(g) + ½O2(g) → H2O(g) (3) C(s, graphite) + 2H2(g) → CH.(g) AH, =-74.6 kJ/mol CO2(g) AH, = -393.5 kJ/mol AH =-241.8 kJ/mol

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) - (2) H2(g) + ½O2(g) → H2O(g) (3) C(s, graphite) + 2H2(g) → CH.(g) AH, =-74.6 kJ/mol CO2(g) AH, = -393.5 kJ/mol AH =-241.8 kJ/mol

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Everything is given .not graded . I attached the equations on separate image
2. Remember, enthalpy is a state function, which allows us to calculate the overall change in enthalpy of a given reaction by summing up the changes from each step along the way. Set up a mathematical equation using variables only (no numbers) for how you determined the change in enthalpy of combustion of methane above. Use the numbers of each equation to keep them separate. Example: AH, (1) + AH, (2) = AH combustion AH combustion fon oolouloting enthalny of combustion using
Transcribed Image Text:2. Remember, enthalpy is a state function, which allows us to calculate the overall change in enthalpy of a given reaction by summing up the changes from each step along the way. Set up a mathematical equation using variables only (no numbers) for how you determined the change in enthalpy of combustion of methane above. Use the numbers of each equation to keep them separate. Example: AH, (1) + AH, (2) = AH combustion AH combustion fon oolouloting enthalny of combustion using
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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