A 12.0 L sample of hydrogen gas has a pressure of 27.0 atm. What volume would this gas occupy at 3.70 atm? Assume ideal behavior.
Constant T.
Use P1V1 = P2V2
To solve this problem, we can use the principle known as Boyle's Law, which states that the pressure and volume of an ideal gas are inversely proportional at constant temperature.
Boyle's Law can be expressed using the following equation:
P1 * V1 = P2 * V2
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 = 27.0 atm (initial pressure)
V1 = 12.0 L (initial volume)
P2 = 3.70 atm (final pressure)
V2 = ?
We can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Plugging in the values, we get:
V2 = (27.0 atm * 12.0 L) / 3.70 atm
To find the value of V2, we can calculate this expression using a calculator or step-by-step calculation:
V2 = (324.0 L atm) / 3.70 atm
V2 ≈ 87.57 L
Therefore, the volume that the hydrogen gas would occupy at 3.70 atm is approximately 87.57 L.