Hydrazine, N₂H4, decomposes according to the following reaction: + N₂ (8) 3 N₂H4 (1) → 4 NH3 (g) (a)The standard enthalpy of formation of hydrazine is 50.42 kJ/mol; calculate AH° for its decomposition Example: (b)Both hydrazine and ammonia burn in oxygen to produce H₂O) and N₂ (g). Write balanced equations for each of these processes and calculate AH° for each of them. On a mass basis (per kg), would hydrazine or ammonia be the better fuel? N₂H4 (1) + O2(g) → 2 H₂O (1) + N₂ (8)
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.
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