Hypergolic propellants are fuels and oxidizers which ignite spontaneously on contact with each other.requiring no ignition source, hypergolics are ideal for spacecraft maneuvering systems as they provide an easy start and restart capability. Also, hypergolics do not pose the storage problems of cryogenic propellants (
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.
- Hypergolic propellants are fuels and oxidizers which ignite spontaneously on contact with each other.requiring no ignition source, hypergolics are ideal for spacecraft maneuvering systems as they provide an easy start and restart capability. Also, hypergolics do not pose the storage problems of cryogenic propellants (e.g., liquid oxygen and hydrogen) as they remain liquid at normal temperatures. This technology was used on the Apollo 11 Mission 40+ years ago.
As part of the testing for a new thruster design, amounts of unsymmetrical dimethyl
hydrazine, or UDMH [(CH3)2N-NH2; MW=60.1 g/mol] were reacted with dinitrogen
tetroxide [N2O4; MW=92.1 g/mol]. The balanced equation for this reaction is shown below:
(CH3)2NNH2(l) + 2 N2O4(g) → 3 N2(g) + 4 H2O(g) + 2 CO2(g)
If 300.5 grams of UDMH are consumed in another test and all of the products gases [N2, water vapor and CO2] are collected into a 100.0-Liter container, determine the following:
The total number of moles of product gases collected into the vessel from this reaction.
What would the total pressure in atmospheres be at 327oC for all of these gases?
What would the partial pressure of the nitrogen gas [N2] be?
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