Estimate the reaction enthalpy for the gas phase reaction of elemental hydrogen (H2) and elemental nitrogen (N2) to form hydrazine (H2N-NH2, a rocket fuel) from the following bond enthalpies: H(breaking H H single bond) = 432 kJ/mol H(breaking N N single bond) = 160 kJ/mol H(breaking N H single bond) = 390 kJ/mol H(breaking N N triple bond) = 945 kJ/mol The balanced equation is given below. In separate lines underneath, write the Lewis structures, the relevant bond enthalpies, and the appropriate multipliers. Then, add up all the contributions to the reaction enthalpy. 2H2+N2---> H2N-NH2
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.
) Estimate the reaction enthalpy for the gas phase reaction of elemental hydrogen (H2) and elemental
nitrogen (N2) to form hydrazine (H2N-NH2, a rocket fuel) from the following bond enthalpies:
H(breaking H H single bond) = 432 kJ/mol
H(breaking N N single bond) = 160 kJ/mol
H(breaking N H single bond) = 390 kJ/mol
H(breaking N N triple bond) = 945 kJ/mol
The balanced equation is given below. In separate lines underneath, write the Lewis structures, the
relevant bond enthalpies, and the appropriate multipliers. Then, add up all the contributions to the
reaction enthalpy.
2H2+N2---> H2N-NH2
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