Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation 4C2H;O2N(s) + 902(lg) 8CO2(g) + 10H20(1I) + 2N2(g) AH°ran = -3857 kJ. Given that AH°(CO2(g)] = -393.5 kJ/mol and AH°;[H2O(1)] = -285.8 kJ/mol, calculate the enthalpy of formation (in kJ/mol) of glycine.
Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation 4C2H;O2N(s) + 902(lg) 8CO2(g) + 10H20(1I) + 2N2(g) AH°ran = -3857 kJ. Given that AH°(CO2(g)] = -393.5 kJ/mol and AH°;[H2O(1)] = -285.8 kJ/mol, calculate the enthalpy of formation (in kJ/mol) of glycine.
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation
4C2H;O2N(s) + 902(lg) 8CO2(g) + 10H20(1I) + 2N2(g) AH°ran = -3857 kJ.
Given that AH°;(CO2(g)] = -393.5 kJ/mol and AH°;[H2O()] = -285.8 kJ/mol, calculate the enthalpy of formation (in kJ/mol) of glycine.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2d7683a8-1fb5-4395-9b85-28d6cf61981b%2Fb61f83e8-4cde-4e2e-ac6a-37d460f43773%2Fm8kiwn_processed.png&w=3840&q=75)
Transcribed Image Text:Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation
4C2H;O2N(s) + 902(lg) 8CO2(g) + 10H20(1I) + 2N2(g) AH°ran = -3857 kJ.
Given that AH°;(CO2(g)] = -393.5 kJ/mol and AH°;[H2O()] = -285.8 kJ/mol, calculate the enthalpy of formation (in kJ/mol) of glycine.
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