Air trapped in a cylinder fitted with a piston occupies 145.7 mL at 1.08 atm pressure. What is the new volume of air when the pressure is increased to 1.34 atm by applying force to the piston?
UseP1V1 = P2V2
117 mL
To determine the new volume of air when the pressure is increased, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature.
Boyle's Law equation:
P1 * V1 = P2 * V2
Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume
Given:
P1 = 1.08 atm
V1 = 145.7 mL
P2 = 1.34 atm
Let's plug in the values into the equation and solve for V2:
1.08 atm * 145.7 mL = 1.34 atm * V2
(1.08 atm * 145.7 mL) / 1.34 atm = V2
V2 ≈ 117.1 mL
Therefore, the new volume of air when the pressure is increased to 1.34 atm is approximately 117.1 mL.
To solve this problem, we can use Boyle's Law, which states that the volume of a given amount of gas is inversely proportional to its pressure, while temperature remains constant.
Boyle's Law equation can be written as:
P1 * V1 = P2 * V2
Where:
P1 = Initial pressure of the gas
V1 = Initial volume of the gas
P2 = Final pressure of the gas
V2 = Final volume of the gas
We are given:
P1 = 1.08 atm
V1 = 145.7 mL
P2 = 1.34 atm (new pressure)
V2 = ? (new volume)
Using Boyle's Law equation, we can solve for V2:
1.08 atm * 145.7 mL = 1.34 atm * V2
Rearranging the equation to solve for V2, we have:
V2 = (1.08 atm * 145.7 mL) / 1.34 atm
Performing the calculation, we get:
V2 ≈ 117.726 mL
Therefore, the new volume of air when the pressure is increased to 1.34 atm is approximately 117.726 mL.