Chapter 2, Problem 2.26NP

(a)

Interpretation Introduction

Interpretation: The value of final q, w, ΔU and ΔH needs to be determined for the isothermal expansion of gas against the constant pressure of $\text{3}\text{.75 }\times {\text{ 10}}^{\text{4}}\text{ Pa}$ , until the volume has doubled.

Concept Introduction: In thermodynamics, a reversible process can be defined as the process which can be reversed without 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.

(b)

Interpretation Introduction

Interpretation:The final q, w, ΔU and ΔH needs to be determined, when gas is cooled at constant volume against constant pressure of $\text{3}\text{.75 }\times {\text{ 10}}^{\text{4}}\text{ Pa}$ .

Concept Introduction: In thermodynamics, a reversible process can be defined as the process which can be reversed without 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.