= One hundred moles of hydrogen gas at 298K are reversibly and isothermally compressed from 30 to 10 L. The van der Waals constants for hydrogen are a = 0.2461 L².atm/mole² and b = 0.02668/mol. In the pressure range of 0 to 1500 atm, the virial equation for hydrogen is PV = RT(1+6.4×10-4P), where P is in atmospheres. (a) Calculate the final pressure and fugacity if (i) Hydrogen behaves as an ideal gas (ii) Hydrogen behaves as a van der Waals gas (iii) Hydrogen behaves according to the virial equation. (b) Calculate the magnitude of the work that must be done on the system to achieve the required change in volume if hydrogen behaves according to the virial equation
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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