At 1 atm, how much energy is required to heat 55.0 g H₂O(s) at -16.0 °C to H₂O(g) at 161.0 °C? Use the heat transfer constantsfound in this table.Show Transcribed TextGHeat-transfer constants for H₂O at 1 atmQuantityEnthalpy of fusion at 0°CHeat Transferper gram333.6 J/g2257 J/gEnthalpy of vaporization at 100°CSpecific heat of solid H₂O (ice)2.087 J/(g-"C)Specific heat of liquid H₂O (water)4.184 J/(g-°C)Specific heat of gaseous H₂O (steam) 2.000 J/(g-°C)per mole6010. J/mol40660 J/molkJ37.60 J/(mol-°C)75.37 J/(mol-°C).36.03 1/(mol-°C)

Answer: Converting ice from -160C to steam at 1610C is 5 step process: 1. Heating of ice 2. melting…

Answered: At 1 atm, how much energy is required…

At 1 atm, how much energy is required to heat 55.0 g H₂O(s) at -16.0 °C to H₂O(g) at 161.0 °C? Use the heat transfer constants found in this table. kJ

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 121QRT

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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

At 1 atm, how much energy is required to heat 55.0 g H₂O(s) at -16.0 °C to H₂O(g) at 161.0 °C? Use the heat transfer constants
found in this table.
Show Transcribed Text
G
Heat-transfer constants for H₂O at 1 atm
Quantity
Enthalpy of fusion at 0°C
Heat Transfer
per gram
333.6 J/g
2257 J/g
Enthalpy of vaporization at 100°C
Specific heat of solid H₂O (ice)
2.087 J/(g-"C)
Specific heat of liquid H₂O (water)
4.184 J/(g-°C)
Specific heat of gaseous H₂O (steam) 2.000 J/(g-°C)
per mole
6010. J/mol
40660 J/mol
kJ
37.60 J/(mol-°C)
75.37 J/(mol-°C).
36.03 1/(mol-°C)

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