When nitric acid reacts with hydrazine (i.e. dinitrogen tetrahydride), nitrogen gas an water are formed. The temperature is constant at 25°C. 4 HNO3(aq) +5 N₂H4(l) → 7 N₂(g) + 12 H₂O(/) Substance HNO3 (aq) H₂O (/) N₂ (g) N₂H4 (/) AH, (kJ/mol) -133.9 -285.8 0 +50.6 a. Calculate AH (in kJ/mol) and AS (in kJ/mol K). b. Calculate AG (in kJ/mol). C. Determine K for this reaction. Sº (kJ/mol K) 0.2669 0.0700 0.1916 0.1212
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.
When nitric acid reacts with hydrazine (i.e. dinitrogen tetrahydride), nitrogen gas and
water are formed. The temperature is constant at 25°C.
4 HNO3(aq) + 5 N2H4(l) " 7 N2(g) + 12 H2O(l)
Substance ΔHf° (kJ/mol) S° (kJ/mol K)
HNO3 (aq) –133.9 0.2669
H2O (l) –285.8 0.0700
N2 (g) 0 0.1916
N2H4 (l) +50.6 0.1212
a. Calculate ΔH° (in kJ/mol) and ΔS° (in kJ/mol K).
b. Calculate ΔG° (in kJ/mol).
c. Determine K for this reaction.
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