THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) → 2X2M (I) + 2DM2 (g) AH°; for X2D (g) = -20.2 kJ/mol AH°; for DM2 (g) = -296.9 kJ/mol AH°f for X2M (1) = -285.9 kJ/mol AH°† for M2 (g) = 0 kJ/mol
THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) → 2X2M (I) + 2DM2 (g) AH°; for X2D (g) = -20.2 kJ/mol AH°; for DM2 (g) = -296.9 kJ/mol AH°f for X2M (1) = -285.9 kJ/mol AH°† for M2 (g) = 0 kJ/mol
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to
ONE decimal place. Do not include the unit.)
2X2D (g) + 3M2 (g) → 2X2M (I) + 2DM2 (g)
AH°; for X2D (g) = -20.2 kJ/mol
AH°; for DM2 (g) = -296.9 kJ/mol
AH°f for X2M (1) = -285.9 kJ/mol
AH°† for M2 (g) = 0 kJ/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F51856ff5-c50e-4b25-815d-4f338def7723%2F86d02ecd-97a9-45e9-a7da-f9c0d2c1213e%2Faj2unet_processed.png&w=3840&q=75)
Transcribed Image Text:THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to
ONE decimal place. Do not include the unit.)
2X2D (g) + 3M2 (g) → 2X2M (I) + 2DM2 (g)
AH°; for X2D (g) = -20.2 kJ/mol
AH°; for DM2 (g) = -296.9 kJ/mol
AH°f for X2M (1) = -285.9 kJ/mol
AH°† for M2 (g) = 0 kJ/mol
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