A sample of oxygen that occupies 1.00x10^6 mL at 575 mm Hg is subjected to a pressure of 1.36 atm. What will the final volume of the sample be if the temperature is held constant?

To solve this problem, you can use the combined gas law, which relates the initial and final conditions of pressure and volume of a gas sample.

The combined gas law formula is given as:

(P1 * V1) / T1 = (P2 * V2) / T2

Where:
- P1 and P2 are the initial and final pressures of the gas sample
- V1 and V2 are the initial and final volumes of the gas sample
- T1 and T2 are the initial and final temperatures of the gas sample

In this problem, the temperature is held constant, so T1 = T2.

Given data:
P1 = 575 mm Hg (convert to atm: 1 atm = 760 mm Hg)
V1 = 1.00x10^6 mL (convert to liters: 1 L = 1000 mL)
P2 = 1.36 atm

Step 1: Convert the given values to the appropriate units
P1 = 575 mm Hg / 760 mm Hg/atm = 0.75658 atm
V1 = 1.00x10^6 mL / 1000 mL/L = 1000 L
P2 = 1.36 atm

Step 2: Plug the values into the combined gas law formula
(0.75658 atm * 1000 L) / T1 = (1.36 atm * V2) / T1

Step 3: Simplify the equation and solve for V2
0.75658 atm * 1000 L = 1.36 atm * V2
756.58 = 1.36 * V2

Divide both sides of the equation by 1.36:
V2 = 756.58 / 1.36

V2 ≈ 556.5 L

Therefore, the final volume of the sample will be approximately 556.5 liters if the temperature is held constant.

Use P1V1=P2V2 and solve for volume.