Chapter 2, Problem 2.6NP

(a)

Interpretation Introduction

Interpretation: The work done needs to be determined if 1.50 mol of an ideal gas sample at initial temperature of $28.5{}^{\text{o}}\text{C}$ expands isothermally with initial and final volume $\text{22}{\text{.5 dm}}^{\text{3}}$ and $\text{75}{\text{.5 dm}}^{\text{3}}$ respectively with an external pressure of $0.498\times {10}^5\text{ Pa}$ .

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,and therefore, the work done will be equal to the change in the internal energy.

(b)

Interpretation Introduction

Interpretation: The work done needs to be determined if 1.50 mol of an ideal gas sample at initial temperature of $28.5{}^{\text{o}}\text{C}$ undergoes isothermal reversible expansion with initial and final volume $\text{22}{\text{.5 dm}}^{\text{3}}$ and $\text{75}{\text{.5 dm}}^{\text{3}}$ respectively

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.