View Policies Current Attempt in Progress The heat of vaporization of mercury is 60.7 kJ/mol. For Hg(1), S° = 76.1 J mol 1 K1, and for Hg(g), S° = 175 J mol 1K-1. Estimate the normal boiling point of liquid mercury. Tea = K oToxtbook and Media

View Policies Current Attempt in Progress The heat of vaporization of mercury is 60.7 kJ/mol. For Hg(1), S° = 76.1 J mol 1 K1, and for Hg(g), S° = 175 J mol 1K-1. Estimate the normal boiling point of liquid mercury. Tea = K oToxtbook and Media

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

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.102QE

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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.

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The heat of vaporization of mercury is 60.7 kJ/mol. For Hg(), S° = 76.1 J mol 1 K 1, and for Hg(g), S° = 175 J mol1 K-1.
Estimate the normal boiling point of liquid mercury.
Tea =
i
K
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Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The nitrogen gas will first condense to liquid at -196oC then the liquid will decrease its temperature to -210oC.
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Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The equilibrium temperature is -260oC.
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Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The magnitude of the heat effect on the flask can be evaluated using the formula C·ΔT.
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? qlost = m·Hv + m·Cp·ΔT.
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