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?

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Answer 1 · 2017-06-11T00:17:11

$260$ $260$ $mm Hg$ $"mm Hg"$

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

$P_{1} V_{1} = P_{2} V_{2}$ $P_1V_1 = P_2V_2$

Since we're trying to find the final pressure ( $P_{2}$ $P_2$ ), let's rearrange the equation to solve for $P_{2}$ $P_2$ :

$P_{2} = \frac{P_{1} V_{1}}{V_{2}}$ $P_2 = (P_1V_1)/(V_2)$

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.