What is the total enthalpy change during the process in which 100.0 g of water at 50.0 °C is cooled to ice at -30.0 °C ? (Assume P= 1.0 atm). Note: COOLING is an EXOTHERMIC PROCESS!!! AH WILL BE NEGATIVE! Solution S.H. water = 4.18 J/g °C Temperature AHfus = 6.01 kJ/mol 50.0 °C 0.0 °C 1 -30.0 °C 2 3 S.H. ice = 2.03 J/g °C 100.0 g H₂O = 5.552 mol H₂O 18.01 g/mol ΔΗ, = SH x Υ x ΔΤ AH₁ = (4.18 J/g °C) (100.0 g)(0.0 - 50.0 °C) = - 20900 J = - 20.9 kJ Energy (J) Thus the total enthalpy change is: AH₂ = -AHfus XY AH₂ = -(6.01 kJ/mol)(5.552 mol) = -33.4 kJ ΔΗ, = SH x Υ x ΔΤ AH3 = (2.03 J/g °C)(100.0 g)(-30.0 -0.00 °C) = 6090 J = -6.09 kJ -20.9 kJ - 33.4 kJ - 6.09 kJ = - 60.4 kJ
What is the total enthalpy change during the process in which 100.0 g of water at 50.0 °C is cooled to ice at -30.0 °C ? (Assume P= 1.0 atm). Note: COOLING is an EXOTHERMIC PROCESS!!! AH WILL BE NEGATIVE! Solution S.H. water = 4.18 J/g °C Temperature AHfus = 6.01 kJ/mol 50.0 °C 0.0 °C 1 -30.0 °C 2 3 S.H. ice = 2.03 J/g °C 100.0 g H₂O = 5.552 mol H₂O 18.01 g/mol ΔΗ, = SH x Υ x ΔΤ AH₁ = (4.18 J/g °C) (100.0 g)(0.0 - 50.0 °C) = - 20900 J = - 20.9 kJ Energy (J) Thus the total enthalpy change is: AH₂ = -AHfus XY AH₂ = -(6.01 kJ/mol)(5.552 mol) = -33.4 kJ ΔΗ, = SH x Υ x ΔΤ AH3 = (2.03 J/g °C)(100.0 g)(-30.0 -0.00 °C) = 6090 J = -6.09 kJ -20.9 kJ - 33.4 kJ - 6.09 kJ = - 60.4 kJ
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.3: Energy And Changes Of State
Problem 1RC: 1. Which of the following processes requires the largest input of energy as heat?
raising the...
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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
Transcribed Image Text:What is the total enthalpy change during the process in which 100.0 g of water at 50.0
°C is cooled to ice at -30.0 °C ? (Assume P = 1.0 atm). Note: COOLING is an
EXOTHERMIC PROCESS!!! AH WILL BE NEGATIVE!
Solution
S.H. water = 4.18 J/g °C
Temperature
AHfus = 6.01 kJ/mol
50.0 °C
0.0 °C
1
-30.0 °C
2
3
S.H. ice = 2.03 J/g °C
100.0 g H₂O = 5.552 mol H₂O
18.01 g/mol
ΔΗ, = SH x Υ x ΔΤ
AH₁ = (4.18 J/g °C)(100.0 g)(0.0 - 50.0 °C)
== - 20900 J - 20.9 kJ
Energy (J)
Thus the total enthalpy change is:
AH₂ = -AHfus XY
AH₂ = -(6.01 kJ/mol)(5.552 mol)
= -33.4 kJ
ΔΗ, = SH x Υ x ΔΤ
AH3 = (2.03 J/g °C)(100.0 g)(- 30.0 - 0.00 °C)
= 6090 J = - 6.09 kJ
-20.9 kJ-33.4 kJ - 6.09 kJ = - 60.4 kJ
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