State what the term ideal gas means.
Two cylinders A and B are linked by a tube of negligible volume, as shown in Fig. 2.1. At the start, 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 $0.34\,\text{mol}$ of gas.
Cylinder B has a fixed volume of $1.6 \times 10^3\,\text{cm}^3$ and contains $0.20\,\text{mol}$ of gas. After tap T is opened, the gas in both cylinders is at pressure $3.9 \times 10^5\,\text{Pa}$. No thermal energy enters or leaves the gas. Determine the final temperature of the gas.
By referring to work done and the change in internal energy, suggest why the temperature of the gas in cylinder A has changed.
Cylinder B has a fixed volume of $1.6 \times 10^3\,\text{cm}^3$ and contains $0.20\,\text{mol}$ of gas. After tap T is opened, the gas pressure in both cylinders is $3.9 \times 10^5\,\text{Pa}$. No thermal energy enters or leaves the gas. Determine the final temperature of the gas.