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.