Three different processes that can occur in an ideal monatomic gas are shown in the P vs V diagram. The paths are labelled as A → B, A → C and A → D. The change in internal energies during these processes are taken as ${E_{AB}}$ , ${E_{AC}}$ and ${E_{AD}}$ and the work done as ${W_{AB}}$ , ${W_{AC}}$ and ${W_{AD}}. The correct relation between these parameters are:

1) ${E_{AB}} = {E_{AC}} = {E_{AD}}, {W_{AB}} > 0, {W_{AC}} = 0, {W_{AD}} < 0$
2) ${E_{AB}} > {E_{AC}} > {E_{AD}} {W_{AB}} < {W_{AC}} < {W_{AD}} $
3) ${E_{AB}} < {E_{AC}} < {E_{AD}} {W_{AB}} > 0, {W_{AC}} > {W_{AD}}$
4)$ {E_{AB}} = {E_{AC}} = {E_{AD}} {W_{AB}} > 0, {W_{AC}} = 0, {W_{AD}} > 0$

Hint: When a monatomic gas behaves optimally, that is, when the gas perfectly obeys the ideal gas equation PV=nRT, it is referred to as an ideal monatomic gas. In thermodynamics, a monatomic gas is one in which the atoms of the gas are not bound to each other such that gas consists of multiple single atoms of particular type. Here, we'll look at the graphed relationship between P and V to get the molar heat capacity.

Complete answer:
The sum of all the energy attributed to the motion of the atoms or molecules within the system is known as internal energy. The rotation, vibration, translation, and interactions of a substance's molecules are examples of microscopic kinds of energy.

Monatomic Gas – Internal energy:
The only source of energy in a monatomic ideal gas (such as helium, neon, or argon) is translational kinetic energy. The equation states that the average translational kinetic energy of a single atom depends only on the temperature of the gas:
${{K}_{avg}}=\dfrac {3}{2} kT$

The average kinetic energy per molecule multiplied by the overall number of molecules, N, gives the internal energy of n moles of an ideal monatomic (one atom per molecule) gas.
\[{{E}_{int}}\text{ }=\text{ }3/2\text{ }NkT\text{ }=\text{ }3/2\text{ }nRT\]

The internal energy is contributed by the three directions (x, y, and z), where n is the number of moles. This is where the concept of energy partition enters; any additional energy supply must also provide (1/2)nRT. As shown, the internal energy of an ideal gas only varies with temperature and the quantity of gas molecules.

We know that the initial and final temperatures for each of the processes are the same.
Therefore, change in internal energy for each process will be equal, i.e.,
$\Delta U=n{{C}_{v}}\Delta T=same$
Thus, ${{E}_{AB}}={{E}_{AC}}={{E}_{AD}}$

Now, work done is given by,
$W=pdV$
For process AB. Volume is increasing
$\Rightarrow {{W}_{AB}}>0$

For process AD, volume is decreasing
$\Rightarrow {{W}_{AD}}<0$

For process AC, volume is constant
$\Rightarrow {{W}_{AC}}=0$

Hence, the option (1) is correct.

Note:These atoms are stable. They rarely form compounds with other atoms because they have fuller outer energy levels. Because it is simple to separate them by overcoming the weak forces of attraction between the atoms, they have low melting and boiling temperatures.