A 1.50-liter sample of dry air in a cylinder exerts a pressure of 3.0 atmospheres at a temperature of 25°C. Wi?
A 1.50-liter sample of dry air in a cylinder exerts a pressure of 3.0 atmospheres at a temperature of 25°C. Without change in temperature, a piston is moved in the cylinder until the pressure in the cylinder is reduced to 1.0 atmosphere. What is the volume of the gas?
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O.k. first off to make things simpler since the Temp doesn't change we can take it out of the equation -
This is Boyle's Law - Before and After volume difference
P1/V1 = P2/V2
These are already in Liters and Atmostpheres so you don't have to convert anything -
So plug in what's given to the equation. 3/1.5 = 1/? Cross multiply and Divide - 1.5(1) / 3 = .5
The volume of the gas is .5 Liters
PV=nRT
1st, make sure to realize that nothing on the right side of the equation will change.
2. when the piston decreases the pressure by 3x (pressure is 1/3 of what it initially was), the Volume will increase by 3x to keep both sides of the equation equal. therefore, the volume will change from 1.50 L to 4.5 L.
Answer = 4.5 L
moral of the story: when you're dealing with the ideal gas law (PV=nRT), both sides will always stay equal to each other. Any change in one variable will result in a proportional increase or decrease of another variable.