Will mark Brainliest The volume of a gas is 3.0 L, the pressure is 1.0 atm, and the temperature is 300 K. A chemist changes one factor while keeping another constant so that the new volume is 2.0 L. Which of the following could be the new conditions?

The final pressure is 0.5 atm, while temperature is kept constant.
The final temperature is 200 K, while pressure remains constant.
The final pressure is 0.2 atm, while temperature is kept constant.
The final temperature is 350 K, while pressure remains constant.

B. The final temperatue is 200K, while pressure remains constant.

Explanation:

I took the test.

According to the ideal gas laws:

When volume increases, pressure decreases if temperature and number of moles is held constant. When volume increases, temperature increases if pressure and number of moles is held constant.

In this case, the volume decreases from 3.0L to 2.0L. That means since the volume decreased, the temperature decreased if the pressure was held constant. OR Since the volume decreased, the pressure increased if the temperature was held constant.

Option A: The final pressure is 0.5 atm, while temperature is kept constant. This is wrong becuase the pressure decreased. Since the volume decreased, the pressure would have increased.Option B: The final temperature is 200 K, while pressure remains constant. This is correct because the the volume decreased and so did the temperature.Option C: The final pressure is 0.2 atm, while temperature is kept constant. This is wrong because the pressure decreased. Since the volume decreased, the pressure would have increased.Option D: The final temperature is 350 K, while pressure remains constant. This is wrong because the temperature increased. Since the volume decreased, the temperature would have decreased.

Answer trigonal pyramidal;