An ideal gas in a box has pressure $p$ and temperature $T$. This box is kept in a vacuum, within a large container.
When the box is punctured, what happens to the temperature of the gas as it expands to fill the entire container?
I was taught that the temperature will remain constant. How is this possible? I understand that the pressure $p$ will decrease and the volume $V$ will increase, but for the temperature $T$ to remain constant, the decrease in $p$ must exactly counterbalance the increase in $V$. Is this the case?