A 4.60*L volume of gas at 845*mm*Hg pressure is expanded such that the new pressure is 368*mm*Hg. To what volume does it expand?

2 Answers
Sep 4, 2017

A measurement of 845*mm*Hg is illegitimate.......

Explanation:

See this old question.......

To solve this question we would use.....

V_2=(P_1V_1)/P_2, but we would insist on kosher units.......

Sep 4, 2017

V_2 = 10.6 "L"

Explanation:

NOTE: Ideally, measurements of pressures greater than 760 "mm Hg" are non-ideal, because mercury barometers only measure up to that value. The equivalent unit, the "torr", should be used if the pressure value exceeds 760 "mm Hg".

We're asked to find the volume necessary for a gas system to exert a pressure of 368 "mm Hg", assuming no change in temperature or amount of gas.

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

ulbar(|stackrel(" ")(" "P_2V_1 = P_2V_2" ")|)" " (constant temperature and quantity)

where

  • P_1 and P_2 are the initial and final pressures of the gas, respectively

  • V_1 and V_2 are the inital and final volumes of the gas, respectively

We know:

  • P_1 = 845 "mm Hg"

  • V_1 = 4.60 "L"

  • P_2 = 368 "mm Hg"

  • V_2 = ?

Let's rearrange the equation to solve for the final volume, V_2:

V_2 = (P_1V_1)/(P_2)

Plugging in known values:

color(red)(V_2) = ((845cancel("mm Hg"))(4.60color(white)(l)"L"))/(368cancel("mm Hg")) = color(red)(ulbar(|stackrel(" ")(" "10.6color(white)(l)"L"" ")|)