Calculate values for the standard reaction enthalpies at 298 K for the reactions in Exercise by using values of the standard enthalpies of formation from the tables in the Resource section. your results with the standard reaction entropies already calculated in that Exercise to
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.
![E3D.4(b) Calculate values for the standard reaction enthalpies at 298 K for the reactions in Exercise
E3C.3(b) by using values of the standard enthalpies of formation from the tables in the Resource section.
Combine your results with the standard reaction entropies already calculated in that Exercise to
determine the standard reaction Gibbs energy at 298 K for each.
Exercise E3C.3(b)
Use data from Tables 2C.3 and 2C.4 to calculate the standard reaction entropy at 298 K of
(i)
Zn(s) + Cu²+ (aq) → Zn²+ (aq) + Cu(s)
(ii)
sucrose [C12H22O11(S)] + 12O2(g) → 12CO2(g) + 11H₂O())
Table 2C.3 Standard enthalpies of formation and combustion of
organic compounds at 298 K*
A.HⓇ/(kJ mol¹)
+49.0
-84.7
Benzene, C,H,(1)
Ethane, C₂H₂(g)
Glucose, C,H,O,(s)
Methane, CH₂(g)
Methanol, CH,OH(1)
* More values are given in the Resource section.
-1274
-74.8
-238.7
AHⓇ/(kJ mol¹)
-3268
-1560
-2808
-890
-721
Table 2C.4 Standard enthalpies of formation of inorganic com-
pounds at 298 K*
H₂O(1)
H₂O(g)
NH,(g)
N₂H (1)
NO₂(g)
N₂O₂(g)
NaCl(s)
KCl(s)
More values are given in the Resource section.
A.HⓇ/(kJ mol™¹)
-285.83
-241.82
-46.11
+50.63
+33.18
+9.16
-411.15
-436.75](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa5be52d7-969f-48e7-912c-c8af10a8f6da%2F13eb7541-ee8a-4300-920f-7d89d11443bc%2Fl1i95fi_processed.png&w=3840&q=75)
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