Standard enthalpy of formation of N(g) is 472 kJ/mol. From this information, estimate the bond enthalpy of N₂. 944 kJ/mol 163 kJ/mol 236 kJ/mol 326 kJ/mol 472 kJ/mol
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.
Introduction
Bond enthalpy is an important physical quantity used to describe the strength of a chemical bond. It is the energy required to break a mole of a given bond in a gaseous state at a given temperature and pressure. The bond enthalpy also quantifies the strength of an intermolecular force, which is ultimately what holds atoms together in molecules. The enthalpy of formation is the energy released when one mole of a compound is formed from its constituent elements in their standard states.
According to the question,
The standard enthalpy of formation of N(g) is given by =
Find- Bond enthalpy for the N2
Step by step
Solved in 3 steps
