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.

Question

Julian Spears

Chemistry

14 November, 08:21

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.

+3

Answers (2)

Know the Answer?

Molly Black · Answer 1

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

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.

Yaritza Walker · Answer 2

The correct answer is at 200C the molecules can overcome intermolecular attractions