Question

15. The ratio PV to nRT is plotted against pressure for CH4 at 0°C and 200°C. Why does the curve for 0°C drop below the horizontal line for an ideal gas whereas the curve for 200°C does not?

A) At 200°C, the molecules can overcome intermolecular attractions.
B) At 200°C, the volume of individual molecules becomes negligible.
C) At 200°C, the forces between molecules become repulsive.

Answer 1

A) At 200 °C, the molecules can overcome intermolecular attractions.

Step-by-step explanation:

At 200 °C, the molecules can overcome intermolecular attractions, so the exerted pressure by the movement of the molecules increases and the positive deviation from ideal gas behavior occurs.