Question

A gas sample occupies 6.00 L at 2.00 atm pressure. At what pressure would the volume be 1.50 L if the temperature remains constant?

1) 0.500 atm
2) 8.00 atm
3) 9.00 atm
4) 12.0 atm

Answer 1

Using Boyle's Law, the pressure required to change the volume of a gas sample from 6.00 L at 2.00 atm to 1.50 L while keeping temperature constant is 8.00 atm. Therefore, correct option is 2.

Step-by-step explanation:

The student is asking about the relationship between gas pressure and volume at constant temperature, which can be explained by Boyle's Law. Boyle's Law states that the pressure of a given mass of an ideal gas is inversely proportional to its volume when the temperature remains constant.

Therefore, if a gas sample occupies 6.00 L at 2.00 atm pressure, and we want to find the pressure when the volume is 1.50 L under constant temperature, we can set up the equation as:

P1 × V1 = P2 × V2

2.00 atm × 6.00 L = P2 × 1.50 L

12.00 atm×L = P2 × 1.50 L

P2 = (12.00 atm×L) / 1.50 L

P2 = 8.00 atm

Thus, the correct answer is 8.00 atm, which is option 2.