Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior. For CO2: a = 3.610 atm dm6 mol-2 b = 0.0429 dm3 mol-1 ΔU= ∫ V2 V1 (an^2/V2)dV If ΔU = -24 J, what is the numeric value of q (in joules)?
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.
Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior.
For CO2:
a = 3.610 atm dm6 mol-2
b = 0.0429 dm3 mol-1
ΔU= ∫ V2 V1 (an^2/V2)dV
If ΔU = -24 J, what is the numeric value of q (in joules)?
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