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20 Consider the reaction: N2(g) + 3H2 (g) = 2NH3 (g) AG°; (NH3) = -17.65kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) Report your answer as a whole number (no places past the decimal point). Do not use scientific notation. Type your answer..

20 Consider the reaction: N2(g) + 3H2 (g) = 2NH3 (g) AG°; (NH3) = -17.65kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) Report your answer as a whole number (no places past the decimal point). Do not use scientific notation. Type your answer..

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter17: Chemcial Thermodynamics
Section: Chapter Questions
Problem 17.20QE: The equilibrium constant for a reaction decreases as temperature increases. Explain how this...
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Type your answer... 20 Consider the reaction: N2(g) + 3H2 (g)2NH3 (g) AG°F (NH3) = -17.65kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) %3D Report your answer as a whole number (no places past the decimal point). Do not use scientific notation. Type your answer...
Transcribed Image Text:Type your answer... 20 Consider the reaction: N2(g) + 3H2 (g)2NH3 (g) AG°F (NH3) = -17.65kJ/mol Determine the equilibrium constant for this reaction at 298.15K. (Hint: Check the stoichiometry of the reaction when you use the Gibbs energy of formation) %3D Report your answer as a whole number (no places past the decimal point). Do not use scientific notation. Type your answer...
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