A sample of oxygen that occupies 2.5 × 10−6 mL at 508 mm Hg is subjected to a pressure of 1.2 atm. What will the final volume of the sample be if the temperature is held constant? Answer in units of mL
P1V1 = P2V2
To find the final volume of the oxygen sample, we can use the combined gas law equation, which relates the initial pressure, initial volume, final pressure, and final volume of a gas when the temperature is held constant.
The combined gas law equation is given by:
(P1 * V1) / (P2 * V2) = 1
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume
Plugging in the given values:
P1 = 508 mm Hg
V1 = 2.5 × 10^(-6) mL
P2 = 1.2 atm (1 atm = 760 mm Hg)
V2 = final volume (what we want to find)
First, let's convert the initial pressure and final pressure to the same unit:
P1 = 508 mm Hg
P2 = 1.2 * 760 mm Hg = 912 mm Hg
Now we can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Substituting the values we have:
V2 = (508 mm Hg * 2.5 × 10^(-6) mL) / 912 mm Hg
Calculating this equation, we find:
V2 = 1.39 × 10^(-9) mL
Therefore, the final volume of the oxygen sample, when subjected to a pressure of 1.2 atm and held at a constant temperature, will be approximately 1.39 × 10^(-9) mL.