# A sample of argon gas at 520 mm Hg expands from 0.150 L to 0.300 L. If the temperature remains constant, what is the final pressure in mm Hg?

Jun 11, 2017

$260$ $\text{mm Hg}$

#### Explanation:

To solve this problem, we can use the pressure-volume relationship of gases, illustrated by Boyle's law:

${P}_{1} {V}_{1} = {P}_{2} {V}_{2}$

Since we're trying to find the final pressure (${P}_{2}$), let's rearrange the equation to solve for ${P}_{2}$:

${P}_{2} = \frac{{P}_{1} {V}_{1}}{{V}_{2}}$

Plugging in known values, we have

P_2 = ((520"mm Hg")(0.150cancel("L")))/(0.300cancel("L")) = color(red)(260 color(red)("mm Hg"

The final pressure is thus $260$ millimeters mercury.