What does the term ideal gas mean?
Two cylinders A and B are linked by a tube of negligible volume, as shown in Fig. 2.1. At the beginning, tap $T$ is closed. The cylinders contain an ideal gas at different pressures.
Cylinder A has a fixed volume of $2.5 \times 10^3\,\text{cm}^3$ and contains gas at pressure $3.4 \times 10^5\,\text{Pa}$ and temperature $300\,\text{K}$. Show that cylinder A contains $0.34$ mol of gas.
Cylinder B has a fixed volume of $1.6 \times 10^3\,\text{cm}^3$ and contains $0.20$ mol of gas. When tap $T$ is opened, the pressure of the gas in both cylinders is $3.9 \times 10^5\,\text{Pa}$. No thermal energy is transferred into or out of the gas. Determine the final temperature of the gas.
Using work done and the change in internal energy, suggest why the temperature of the gas in cylinder A has altered.