The value of q, w, Δ and Δ for the process in which the temperature of 1.75 moles of an ideal gas increases from 10 .2 ° C to 48 .6 ° C needs to be determined, when the gas is compressed adiabatically. Concept Introduction: In thermodynamics , a reversible process can be defined as the process which can be reversed to its original state. Hence in reversible processes, both the system and surroundings are returned to their initial states. In general, all reversible processes are ideal processes and cannot occur naturally. On the contrary, an irreversible process cannot come back to its initial condition. All spontaneous processes in nature are irreversible processes. In an adiabatic process the heat change is zero therefore the work done will be equal to the change in the internal energy.

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Chapter 2, Problem 2.2NP

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Interpretation: The value of q, w, Δ and Δ for the process in which the temperature of 1.75 moles of an ideal gas increases from 10.2°C to 48.6°C needs to be determined, when the gas is compressed adiabatically.

Concept Introduction: In thermodynamics, a reversible process can be defined as the process which can be reversed to its original state.

Hence in reversible processes, both the system and surroundings are returned to their initial states. In general, all reversible processes are ideal processes and cannot occur naturally.

On the contrary, an irreversible process cannot come back to its initial condition. All spontaneous processes in nature are irreversible processes.

In an adiabatic process the heat change is zero therefore the work done will be equal to the change in the internal energy.

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