At constant temperature, a #3.8*L# volume of gas at #765*mm*Hg#, was expanded to give a pressure of #0.500*atm#. What is the new volume?

1 Answer
May 4, 2017

Answer:

#P_1V_1=P_2V_2# under conditions of constant temperature.

Explanation:

We need to know that #1*atm# will support a column of mercury that is #760*mm# high, and thus a mercury column may used as a highly visual measurement of pressure:

#1*atm-=760*mm*Hg# (note that given the schemozzle that occurs when you spill mercury in the lab, you really should not put mercury under a pressure of MORE than 1 atmosphere). Here.......

#P_1=(765*mm*Hg)/(760*mm*Hg*atm^-1)=1.01*atm.#

We solve for #V_2=(P_1V_1)/P_2=(1.01*atmxx3.8*L)/(0.500*atm)=7.60*L#