An isolated system is that which can exchange energy but not matter with the surroundings.

Consider the given diagram. An ideal gas is contained in a chamber (left) of volume $V$ and is at an absolute temperature $T.$ It is allowed to rush freely into the right chamber of volume $V$ which is initially vacuum. The whole system is thermally isolated. What will be the final temperature, if the equilibrium has been attained?

Consider the following thermodynamical variables
(i) Pressure
(ii) Internal Energy
(iii) Volume
(iv) Temperature

Out of these, the intensive variable(s) is (are)

Pressure versus temperature graph of an ideal gas at constant volume $V$ is shown by the straight-line $A$. Now mass of the gas is doubled and the volume is halved then the corresponding pressure versus temperature graph will be shown by the line

The pressure versus temperature graph of an ideal gas is shown in the figure below. If the density of gas at point $A$ is ${\rho }_0$, then the density of the gas at point $B$ will be

Three different processes that can occur in an ideal monoatomic gas are shown in the $P$ vs $V$ diagram. The paths are labelled as $A\to B,A\to C$ and $A\to D$. The change in internal energies during these process 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:

Some of the thermodynamic parameters are state variables while some are process variables. Some grouping of the parameters are given. Choose the correct one