One mole of an ideal gas is contained at 273 K and a pressure of 1 atm. The addition of 3088 joules of heat to the gas at constant pressure causes 817 Joules of work to be done during the expansion. Calculate: (a) The final states (volume and temperature) of the gas, (b) The change in the internal energy (c) The change in the enthalpy and (d) The values of cv and cp for idealgas (R: 0.082 liter atm/degree.mole or 8.314 Joules/degree mole) (1L.atm =101.325 J)
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.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
