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 once the equilibrium has been attained?

In a thermodynamic process of uncontrolled change satisfying the equation $Q=W=0$,where $Q$ is heat supplied and $W$ is work done,the process is:

Two cylinders $A$ and $B$ of equal capacity are connected to each other via a stopcock. $A$ contains a gas at standard temperature and pressure. $B$ is completely evacuated. The entire system is thermally insulated. The stopcock is suddenly opened. Answer the following :
$(a)$ What is the final pressure of the gas in $A$ and $B$?
$(b)$ What is the change in internal energy of the gas?
$(c)$ What is the change in the temperature of the gas?
$(d)$ Do the intermediate states of the system (before settling to the final equilibrium state) lie on its $P-V-T$ surface?

In case of free expansion, which one of the following statements is $\underline{\text{WRONG}}$?

When a gas in a vacuum chamber expands suddenly,which of the following is true?

Which thermodynamic process is quasi-static and does not dissipate energy?