Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: 2X2D (g) + 3M2 (g) → 2X2M (1) + 2DM2 (g) AH°F for X2D (g) -22.7 kJ/mol AH°F for DM2 (g) = -292.8 kJ/mol AH°F for X2M (1) = -289.3 kJ/mol AH°f for M2 (g) = 0 kJ/mol

Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: 2X2D (g) + 3M2 (g) → 2X2M (1) + 2DM2 (g) AH°F for X2D (g) -22.7 kJ/mol AH°F for DM2 (g) = -292.8 kJ/mol AH°F for X2M (1) = -289.3 kJ/mol AH°f for M2 (g) = 0 kJ/mol

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

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.81QE

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Question

Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction:
2X2D (g) + 3M2 (g) → 2X2M (1) + 2DM2 (g)
AH°F for X2D (g) = -22.7 kJ/mol
AH°f for DM2 (g) = -292.8 kJ/mol
AH°F for X2M (1) = -289.3 kJ/mol
AH°f for M2 (g) = 0 kJ/mol

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