If the temperature of a system of one mole of an ideal gas is changed from T1°C to T2-2T1 °C is accompanied by a change in internal energy of 4000J, (a)Calculate the change in internal energy of the gas for doubling of the temperature at constant volume. (b) Is there any heat supplied into or out of the system? (c) Does this quantity of heat correspond to the change in enthalpy of the gas. Volume (L) The figure above depicts the two processes. Use this to show that for an ideal gas Cp- CV = nR Where Cp is the heat capacity at constant pressure and Cy is the heat capacity at constant volume. State all the assumptions made if any. Pressure (atm)
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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