a sample of carbon dioxide has a volume of 25.0L at 5.80 x 10^2 mmHg. what pressure would be needed to increase the volume to 55.5 L? assume constant temperature
P1V1 = P2V2
To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, assuming constant temperature. The formula for Boyle's Law is:
P1 * V1 = P2 * V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume
Given:
V1 = 25.0 L
P1 = 5.80 x 10^2 mmHg
V2 = 55.5 L
We can plug in these values into Boyle's Law equation and solve for P2:
P1 * V1 = P2 * V2
(5.80 x 10^2 mmHg) * (25.0 L) = P2 * (55.5 L)
Simplifying the equation:
(5.80 x 10^2 mmHg * 25.0 L) / 55.5 L = P2
Calculating the result:
P2 = (5.80 x 10^2 mmHg * 25.0 L) / 55.5 L
P2 ≈ 260.36 mmHg
Therefore, a pressure of approximately 260.36 mmHg would be needed to increase the volume to 55.5 L.