A sample of Argon gas at standard pressure occupies 1000 mL. At constant temperature, what volume does the gas occupy if the pressure increases to 800 mm Hg?

950

P1V1 = P2V2

1000 divided by 600

To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. Mathematically, it can be expressed as:

(P1 * V1) = (P2 * V2)

Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume

In this case, the initial pressure is the standard pressure, and the initial volume is given as 1000 mL. The final pressure is 800 mm Hg, and we need to find the final volume.

Let's plug in the values into the equation and solve for V2:

(P1 * V1) = (P2 * V2)

(1 atm * 1000 mL) = (800 mm Hg * V2)

Next, let's convert the units so that they are consistent:

1 atm = 760 mm Hg (standard pressure)

(760 mm Hg * 1000 mL) = (800 mm Hg * V2)

Now, we can solve for V2:

760,000 mm Hg mL = 800 mm Hg * V2

V2 = (760,000 mm Hg mL) / (800 mm Hg)

V2 = 950 mL

Therefore, when the pressure increases to 800 mm Hg, the volume of the Argon gas occupies is 950 mL.