At 2.0 atm pressure, the volume of a gas is 4.0 L. If the pressure is reduced to 1.0 atm while keeping the temperature constant, what will be the new volume of the gas?
In this scenario, we have a gas at an initial pressure of 2.0 atm and an initial volume of 4.0 L. We are told that the temperature is constant throughout the process.
The question asks us to determine the new volume of the gas if the pressure is reduced to 1.0 atm. To do this, we can use the Boyle's Law.
Boyle's Law states that if the temperature of a gas remains constant, then the pressure and volume of the gas are inversely proportional. In other words, as the pressure decreases, the volume increases.
Using Boyle's Law, we can set up the following equation:
P1 * V1 = P2 * V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume (what we need to find)
Substituting the given values into the equation, we have:
(2.0 atm) * (4.0 L) = (1.0 atm) * (V2)
Simplifying the equation:
8.0 L atm = V2 * 1.0 atm
Since the pressure and volume are inversely proportional, we can solve for V2 by dividing both sides of the equation by 1.0 atm:
V2 = 8.0 L
Therefore, the new volume of the gas when the pressure is reduced to 1.0 atm while keeping the temperature constant will be 8.0 L.