Determine the heat involved in the combustion of liquid hydrazine by using the following reactions. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ) ΔH°= –1013 kJ/mol N2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –317 kJ/mol 2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –142.9 kJ/mol H2(g) + ½ O2(g) → H2O(ℓ) ΔH°= –285.8 kJ/mol Then, Launching a small spacecraft to study Jupiter required approximately 28 million kJ. Assume that hydrazine was the only fuel. What mass of hydrazine, in kilograms, was needed for the launch?
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.
Determine the heat involved in the combustion of liquid hydrazine
by using the following reactions.
2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ) ΔH°= –1013 kJ/mol
N2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –317 kJ/mol
2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ) ΔH°= –142.9 kJ/mol
H2(g) + ½ O2(g) → H2O(ℓ) ΔH°= –285.8 kJ/mol
Then, Launching a small spacecraft to study Jupiter required
approximately 28 million kJ. Assume that hydrazine was the only
fuel. What mass of hydrazine, in kilograms, was needed for the
launch?
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