2. (a) The heat of combustion of liquid benzaldehyde (C6H5CHO) is -3393 kJ/mole, and that ofliquid 2,4,6-cycloheptatrien-1-one (C₂H6O) is -3470 kJ/mole. Assume that bothcombustions result in products, CO2 and H₂O, that are entirely in the gas phase. Usingthe standard chemical equation for the combustion of a hydrocarbon, find the heats offormation (in kJ/mol) for both benzaldehyde and 2,4,6-cycloheptatrien-1-one in theliquid phase.(b) Consider the isomerization from 2,4,6-cycloheptatrien-1-one to benzaldehyde. What isthe enthalpy change (in kJ/mol) for this reaction? Is it endothermic or exothermic?(c) If ArxnS = -18 J/mol-K for the isomerization reaction, find ArxnG at 350 K (in kJ/mol) anddetermine if it is spontaneous in the liquid phase at this temperature. For thiscalculation, you may assume that ArxnH and ArxnS are constant between 300 and 350 K.

(a) The heat of combustion of liquid benzaldehyde is given to be -3393 kJ/mol while that of liquid…

The heat of combustion of liquid benzaldehyde (C6H5CHO) is -3393 kJ/mole, and that of liquid 2,4,6-cycloheptatrien-1-one (C7H6O) is -3470 kJ/mole. Assume that both combustions result in products, CO₂ and H₂O, that are entirely in the gas phase. Using the standard chemical equation for the combustion of a hydrocarbon, find the heats of formation (in kJ/mol) for both benzaldehyde and 2,4,6-cycloheptatrien-1-one in the liquid phase. Consider the isomerization from 2,4,6-cycloheptatrien-1-one to benzaldehyde. What is the enthalpy change (in kJ/mol) for this reaction? Is it endothermic or exothermic? If ArxnS = -18 J/mol-K for the isomerization reaction, find ArxnG at 350 K (in kJ/mol) and determine if it is spontaneous in the liquid phase at this temperature. For this calculation, you may assume that ArxnH and ArxnS are constant between 300 and 350 K.

The heat of combustion of liquid benzaldehyde (C6H5CHO) is -3393 kJ/mole, and that of liquid 2,4,6-cycloheptatrien-1-one (C7H6O) is -3470 kJ/mole. Assume that both combustions result in products, CO₂ and H₂O, that are entirely in the gas phase. Using the standard chemical equation for the combustion of a hydrocarbon, find the heats of formation (in kJ/mol) for both benzaldehyde and 2,4,6-cycloheptatrien-1-one in the liquid phase. Consider the isomerization from 2,4,6-cycloheptatrien-1-one to benzaldehyde. What is the enthalpy change (in kJ/mol) for this reaction? Is it endothermic or exothermic? If ArxnS = -18 J/mol-K for the isomerization reaction, find ArxnG at 350 K (in kJ/mol) and determine if it is spontaneous in the liquid phase at this temperature. For this calculation, you may assume that ArxnH and ArxnS are constant between 300 and 350 K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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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Question

2. (a) The heat of combustion of liquid benzaldehyde (C6H5CHO) is -3393 kJ/mole, and that of
liquid 2,4,6-cycloheptatrien-1-one (C₂H6O) is -3470 kJ/mole. Assume that both
combustions result in products, CO2 and H₂O, that are entirely in the gas phase. Using
the standard chemical equation for the combustion of a hydrocarbon, find the heats of
formation (in kJ/mol) for both benzaldehyde and 2,4,6-cycloheptatrien-1-one in the
liquid phase.
(b) Consider the isomerization from 2,4,6-cycloheptatrien-1-one to benzaldehyde. What is
the enthalpy change (in kJ/mol) for this reaction? Is it endothermic or exothermic?
(c) If ArxnS = -18 J/mol-K for the isomerization reaction, find ArxnG at 350 K (in kJ/mol) and
determine if it is spontaneous in the liquid phase at this temperature. For this
calculation, you may assume that ArxnH and ArxnS are constant between 300 and 350 K.

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