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.
how do I calculate literature delta H using the list of reaction provided?
![Compare your experimental AH values for the reactions studied in the lab with the literature
values for these reactions. If any of the observed results deviate from the literature values by a
DISCUSSION
significant amount (i.e.> 106), determine and explain how a source of experimental error would
lead to the observed difference in each case.
Enthalpy of Reaction Data for the Solution Calorimetry Lab
The following table should provide all the data you need to calculate the literature enthalpy of
reaction volues for the reactions studied in the lob today. The lines in the table divide up the
data given to (roughly) correspond with what is needed for the experiments performed,
although it may be necessary to use a given data item more than once. All enthalpies of
formation are for reactions carried out under standard conditions at a temperature of 25°C.
Reaction
AH° (kJ)
O:lg) + Hale) + Na(s)
I Hale) + Clale)
Hole) + Nalg) + 글o8)
-470.11
NaOH(aq)
HCI(aq)
-167.16
HNO(aq)
-207.4
Hals) + Ozle)
-285.83
Chle) + Na(s)
NaCl(aq)
-407.3
I Nale) + Osle) + Na(s)
NANO,(aq)
-447.5
2Na(s) + Sals) + O:lg)
NazS,Os(aq)
-1132.4
2Na(s) + 4 Suls) + Osle)
NazS,Os(s)
-1123.
2Na(s) + Sals) + 40;(g) + SH:le)
NaS,OySH;O(s)
-2607.9
2e+ Sals) + } 0:l8)
S,O, (aq)
-652.3
Na(s)
Na"(aq) +e
-240.1
Mg(s) + Clale)
MgCla(aq)
-801.15
Mg(s) + O:le)
H:le) + Pals) + 20;(8)
e+ Halg) + Pals) + 20:(g)
MgO(s)
-601.70
HPO.(aq)
-1288.3
HPO. (aq)
-1296.3
HPO (aq)
2e+ Hale) + Pals) + 20;lg)
-1292.1
PO (aq)
3e" + Pals) + 20:(g)
-1277.4
H"(aq) +e
0.0
99](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F182fc570-9c1f-4672-95f0-0f5ff5e56e31%2F29d965ca-0c13-463a-bf43-5048c2de7074%2Fj17s8ta_processed.png&w=3840&q=75)
![SUMMARY TABLE:
Reaction
ΔΗ(1)
ΔΗ(2)
AH(avg)
Literature AH
A) HCl + NaOH
Bi) NazS203 + H2О
B2) NazS2O3·5H2O +
H2O
C) Mg + HCl
D) MgO + HCl
E) HРО4 + NaOH
Ей) Н3РО4 + 2NaOH
Ei) HaPOд + 3NaOH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F182fc570-9c1f-4672-95f0-0f5ff5e56e31%2F29d965ca-0c13-463a-bf43-5048c2de7074%2F6ljblja_processed.png&w=3840&q=75)
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