Given the listed average bond energies, calculate the enthalpy change for the production of 48 g of methanol by thereaction:CO2(g) + 3 H2(g) CH3OH(g) + H2O(g)C-0/360 kJ/molC=0/736 kJ/molH-H/436 kJ/molH-O/464 kJ/molH-C/414 kJ/molSeçtiğiniz cevabın işaretlendiğini görene kadar bekleyiniz. Soruyu boş birakmak isterseniz işaretledığiniz seçeneğe tekrar tiklayınız.17:06amak için buraya yazınTUR28.04.2021ort scdeletehomeendnumlock

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Given the listed average bond energies, calculate the enthalpy change for the production of 48 g of methanol by the reaction:

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 5.79QE

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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

Given the listed average bond energies, calculate the enthalpy change for the production of 48 g of methanol by the
reaction:
CO2(g) + 3 H2(g) CH3OH(g) + H2O(g)
C-0/360 kJ/mol
C=0/736 kJ/mol
H-H/436 kJ/mol
H-O/464 kJ/mol
H-C/414 kJ/mol
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