Question

determine whether each of the following statements regarding real gases (compared to ideal gases) are true or false.
gases become less ideal at higher pressure. -- ◊
the actual volume available for a gas particle is smaller than the total volume of the container (v). -- ◊
the volume of the gas particles becomes more significant at lower pressure. -- ◊
the attractive forces that exist between gas particles cause the measured pressure of a gas to be higher than that predicted by the ideal gas law. -- ◊
the attractive forces between gas molecules are negligible and can be ignored at higher temperatures. -- ◊

Explanation:

• Statement 1: At higher pressure, gas particles are closer. Inter - particle forces and particle volume matter more, so gases are less ideal. True.
• Statement 2: Gas particles have volume. So, the actual volume available for a gas particle \( V_{available}=V - V_{particles}\), where \( V\) is the container volume. True.
• Statement 3: At lower pressure, gas particles are farther apart. The volume of gas particles is less significant compared to the container volume. False.
• Statement 4: Attractive forces between gas particles reduce the force of collision with the container walls. So, the measured pressure is lower than ideal. False.
• Statement 5: At higher temperatures, gas particles have higher kinetic energy. Attractive forces are overcome, so they are negligible. True.

Answer:

1. True
2. True
3. False
4. False
5. True