A sample of methane gas at room temperature has a pressure of 1.50 atm and a volumne of 10.5 L. If the temperature is kept constant, what will be the new volume if the pressure is increased to 2.00 atm?
P1V1 = P2V2
To determine the new volume of the methane gas, we can use Boyle's Law. Boyle's Law states that at a constant temperature, the pressure and volume of a gas are inversely proportional.
Boyle's Law can be mathematically expressed as: P1 * V1 = P2 * V2
Where:
P1 is the initial pressure (1.50 atm)
V1 is the initial volume (10.5 L)
P2 is the final pressure (2.00 atm)
V2 is the final volume (unknown)
We can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Now we can substitute the given values into the equation:
V2 = (1.50 atm * 10.5 L) / 2.00 atm
Calculating this equation gives us:
V2 = 7.875 L
Therefore, the new volume of the methane gas, when the pressure is increased to 2.00 atm, will be 7.875 L.