What is the pressure in #mm*Hg# if a #4.0*g# mass of oxygen gas at #303*K# was confined to a container whose volume of #3000*mL#?

1 Answer
anor277
Jun 28, 2017

#P=1.04*atm.......#

Explanation:

We use the Ideal Gas Equation, to give.....

#P=(nRT)/V=((4.00*g)/(32.00*g*mol^-1)xx0.0821*(L*atm)/(K*mol)xx303*K)/(3000*mLxx10^-3*L*mL^-1)#

#=1.04*atm#

Now had the pressure been UNDER #1*atm# I could use the relationship #1*atm-=760*mm*Hg#; i.e. an atmosphere will support a column of mercury that is so high. You do not measure a pressure that is greater than #1*atm# in #mm*Hg#. Whoever set this problem was ignorant.........

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