A #0.275*L# volume of an unspecified gas exerts a pressure of #732.6*mm*Hg# at a temperature of #-28.2# #""^@C#. What is the molar quantity of this gas?

1 Answer
Apr 3, 2017

Answer:

Approx. #0.013*mol#

Explanation:

We need to know that #1*atm# will support a column of mercury #760*mm# high, and thus we can use the length of a mercury column to express pressure.

And thus #P=(732.6*mm*Hg)/(760*mm*Hg*atm^-1)=??*atm#

And we use the #"Ideal Gas Law"#, #n=(PV)/(RT)#

#n=(PV)/(RT)=((732.6*mm*Hg)/(760*mm*Hg*atm^-1)xx0.275*L)/(0.0821*L*atm*K^-1*mol^-1xx245*K)=#

#1.32xx10^-2*mol.#

Why did I change the temperature to #"degrees Kelvin"#?