A 1.5 liter flask is filled with nitrogen at a pressure of 12 atmospheres. What size flask would be required to hold this gas at a pressure of 2.0 atmosphere?
P1 V1 = P2 V2
12* 1.5 = 2* V2
that assumes your pressures are abolute. If they are gage pressures then
13 * 1.5 = 3 * V2
1.5 liter flask is filled with nitrogen at pressure of 12 atmosphere. What size would be required to hold this gas at a pressure of 2.0 atmosphere?
To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.
Boyle's Law can be mathematically represented as: P1 * V1 = P2 * V2
Where:
P1 = initial pressure (12 atm)
V1 = initial volume (1.5 L)
P2 = final pressure (2.0 atm)
V2 = final volume (unknown)
To find the final volume (V2), we can rearrange the equation as follows:
V2 = (P1 * V1) / P2
Plugging in the given values, we have:
V2 = (12 atm * 1.5 L) / 2.0 atm
V2 = 9 L
Therefore, a flask with a volume of 9 liters would be required to hold the nitrogen gas at a pressure of 2.0 atmospheres.