A 3.0 L container holds a sample of oxygen gas at 1.5 atm pressure. If the pressure increases to 2.0 atm and the temperature remains constant, what is the new volume of the container?
To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when the temperature and amount of gas remain constant. The formula for Boyle's Law is P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
In this case, we are given:
P1 = 1.5 atm (initial pressure)
V1 = 3.0 L (initial volume)
P2 = 2.0 atm (final pressure)
We need to find V2 (final volume).
Using the Boyle's Law formula, we can rearrange it to solve for V2:
V2 = (P1 * V1) / P2
Plugging in the given values:
V2 = (1.5 atm * 3.0 L) / 2.0 atm
Simplifying the equation:
V2 = 4.5 L / 2.0
Calculating the final volume:
V2 = 2.25 L
Therefore, the new volume of the container is 2.25 L when the pressure increases to 2.0 atm, assuming the temperature remains constant.
P1V1 = P2V2
Plug in the values and turn the crank for the answer.
I don't want to confuse you but I doubt that the volume of the CONTAINER changed. After all, a container has a certain volume when it's manufactured. However, the VOLUME that is holding the gas will change.