C6H5OH(s) + 7 O2(g) ---> 6 CO2(g) + 3H₂O(1)When a 2.000-gram sample of pure phenol, C6H5OH(s), is completely burned according to the equation above,64.98 kilojoules of heat is released. Use the information in the table below to answer the questions that follow.Standard Heat ofSubstance Formation, AHºf,at 25°C (kJ/mol)C(graphite)CO₂(g)H₂(g)H₂O(1)O₂(g)C6H5OH(s)Absolute Entropy, Sº,at 25°C (J/mol-K)0.00f 5.69213.6130.669.91205.0144.0-395.5w0.00-285.850.00?070107(0042 (5(O(a) Calculate the molar heat of combustion of phenol inkilojoules per mole at 25°C.(b) Calculate the standard heat of formation, AH°f, ofphenol in kilojoules per mole at 25°C.166(c) Calculate the value of the standard free-energy change, AG° for the combustion of phenol at 25°C.

Given that 2.000 g of phenol releases 64.98 kJ heat, To obtain the molar heat , we need to convert…

C6H5OH(s) + 7 O2(g) ---> 6 CO2(g) + 3H₂O(1) H When a 2.000-gram sample of pure phenol, C6H5OH(s), is completely burned according to the equation above, 64.98 kilojoules of heat is released. Use the information in the table below to answer the questions that follow. Standard Heat of Substance Formation, AHᵒf, at 25°C (kJ/mol) C(graphite) CO₂(g) H₂(g) H₂O(1) O₂(g) C6H5OH(s) 0.00 -395.5 0.00 -285.85 0.00 ? Absolute Entropy, Sº, at 25°C (J/mol-K) 5.69 213.6 130.6 69.91 205.0 144.0 01 (a) Calculate the molar heat of combustion of phenol in kilojoules per mole at 25°C. (b) Calculate the standard heat of formation, AHᵒf, of phenol in kilojoules per mole at 25°C. plastov (0) (c) Calculate the value of the standard free-energy change, AG° for the combustion of phenol at 25°C.

C6H5OH(s) + 7 O2(g) ---> 6 CO2(g) + 3H₂O(1) H When a 2.000-gram sample of pure phenol, C6H5OH(s), is completely burned according to the equation above, 64.98 kilojoules of heat is released. Use the information in the table below to answer the questions that follow. Standard Heat of Substance Formation, AHᵒf, at 25°C (kJ/mol) C(graphite) CO₂(g) H₂(g) H₂O(1) O₂(g) C6H5OH(s) 0.00 -395.5 0.00 -285.85 0.00 ? Absolute Entropy, Sº, at 25°C (J/mol-K) 5.69 213.6 130.6 69.91 205.0 144.0 01 (a) Calculate the molar heat of combustion of phenol in kilojoules per mole at 25°C. (b) Calculate the standard heat of formation, AHᵒf, of phenol in kilojoules per mole at 25°C. plastov (0) (c) Calculate the value of the standard free-energy change, AG° for the combustion of phenol at 25°C.

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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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

C6H5OH(s) + 7 O2(g) ---> 6 CO2(g) + 3H₂O(1)
When a 2.000-gram sample of pure phenol, C6H5OH(s), is completely burned according to the equation above,
64.98 kilojoules of heat is released. Use the information in the table below to answer the questions that follow.
Standard Heat of
Substance Formation, AHºf,
at 25°C (kJ/mol)
C(graphite)
CO₂(g)
H₂(g)
H₂O(1)
O₂(g)
C6H5OH(s)
Absolute Entropy, Sº,
at 25°C (J/mol-K)
0.00f 5.69
213.6
130.6
69.91
205.0
144.0
-395.5w
0.00
-285.85
0.00
?
070107
(0042 (5
(O
(a) Calculate the molar heat of combustion of phenol in
kilojoules per mole at 25°C.
(b) Calculate the standard heat of formation, AH°f, of
phenol in kilojoules per mole at 25°C.
166
(c) Calculate the value of the standard free-energy change, AG° for the combustion of phenol at 25°C.

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