a. Calculate the heat required to melt 5.87 g of benzene at its normal melting point. Heat of fusion (benzene) = 9.92 kJ/mol %3D Heat = %3D b. Calculate the heat required to vaporize 5.87 g of benzene at its normal boiling point. Heat of vaporization (benzene) = 30.7 kJ/mol Heat = kJ

a. Calculate the heat required to melt 5.87 g of benzene at its normal melting point. Heat of fusion (benzene) = 9.92 kJ/mol %3D Heat = %3D b. Calculate the heat required to vaporize 5.87 g of benzene at its normal boiling point. Heat of vaporization (benzene) = 30.7 kJ/mol Heat = kJ

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 15E: The melting point of H2O(s) is O C. Would you expect the melting point of H2S(s) to be 85 C, O C, or...

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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

a. Calculate the heat required to melt 5.87 g of benzene at its normal melting point.
Heat of fusion (benzene) = 9.92 kJ/mol
Heat =
b. Calculate the heat required to vaporize 5.87 g of benzene at its normal boiling point.
Heat of vaporization (benzene) = 30.7 kJ/mol
Heat =
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