The compressibility of a gas is less than unity at STP. Therefore — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

I need to see the options to provide a complete explanation. However, I can explain the key concept: **Compressibility Factor Analysis:** The compressibility factor is defined as: $$Z = \frac{PV}{nRT}$$ When $Z < 1$ at STP, this means: $$PV < nRT$$ **Physical Interpretation:** - $Z < 1$ indicates the gas is **more easily compressed** than an ideal gas - This occurs because **intermolecular attractive forces dominate** over repulsive forces - The gas molecules experience net attractions, reducing the pressure exerted on container walls **Common conclusions for $Z < 1$:** - The gas deviates negatively from ideal behavior - Real pressure is less than ideal pressure for the same volume and temperature - Attractive forces > Repulsive forces at these conditions - The gas will liquefy more readily under compression **Likely correct option B** (without seeing all choices) probably states: - "Intermolecular attractive forces dominate" - OR "The gas deviates negatively from ideality" - OR "The real pressure is less than calculated ideal pressure" If you provide the complete options, I can confirm which specific statement is option B and verify it's correct.