A sample of gas has an initial volume of 20.9 L at a pressure of 1.4 atm
If the sample is compressed to a volume of 12.9 L: , what will its pressure be? (Assume constant temperature.)
Thank you
Assuming the gas is ideal, we can use Boyle's Law:
P1 * V1 = P2 * V2
where P is pressure and V is volume.
Substituting,
1.4 * 20.9 = P2 * 12.9
P2 = ?
Units in atm. Hope this helps~ :3
To find the new pressure of the gas sample after it is compressed, we can use Boyle's Law. Boyle's Law states that the product of the initial volume and pressure of a gas is equal to the product of its final volume and pressure, assuming the temperature remains constant.
The formula for Boyle's Law is: P1 * V1 = P2 * V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure (what we're trying to find)
V2 = final volume
Given:
P1 = 1.4 atm
V1 = 20.9 L
V2 = 12.9 L
Let's substitute the known values into the equation and solve for P2:
(1.4 atm) * (20.9 L) = P2 * (12.9 L)
Multiply:
29.26 atm*L = 12.9 P2 * L
Divide both sides by 12.9 L:
29.26 atm = P2
Therefore, when the gas is compressed to a volume of 12.9 L, its pressure will be 29.26 atm.