calculate the value of ΔHf for Mg2+ using the 28.57 kj/mol and the table 8.1 (attached is table 8.1) 1.SpeciesNH4Cl (s)NH4NO3 (s)KCI (s)NaCl (s)KI (s)Nal (s)MgCl2 (s)Cl (aq). I (aq)NO3 (aq)c (J/°C.g)1.571.7410.688 6/sb 010100-436.75hami "mnds!317AfH (kJ/mol)-314.43-356.56A0.864in0.319 eminalsa ed-327.90qoist to nás g0.3480.750-411.15-287.78-641.32-167.16-55.2-111.3

To calculate the standard molar enthalpy of formation (ΔHf) for Mg2+ (magnesium ion), we need to…

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calculate the value of ΔHf for Mg2+ using the 28.57 kj/mol and the table 8.1 (attached is table 8.1)

Chemistry for Engineering Students

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ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 3CO

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Concept explainers

Thermochemistry

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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

calculate the value of ΔHf for Mg2+ using the 28.57 kj/mol and the table 8.1 (attached is table 8.1)

1.
Species
NH4Cl (s)
NH4NO3 (s)
KCI (s)
NaCl (s)
KI (s)
Nal (s)
MgCl2 (s)
Cl (aq)
. I (aq)
NO3 (aq)
c (J/°C.g)
1.57
1.74
10.688 6/sb 010100-436.75
hami "mnds!
317
AfH (kJ/mol)
-314.43
-356.56
A
0.864
in
0.319 eminalsa ed-327.90
qoist to nás g
0.348
0.750
-411.15
-287.78
-641.32
-167.16
-55.2
-111.3

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