A 0.275*L0.275⋅L volume of an unspecified gas exerts a pressure of 732.6*mm*Hg732.6⋅mm⋅Hg at a temperature of -28.2−28.2 ""^@C∘C. What is the molar quantity of this gas?

1 Answer
anor277
Apr 3, 2017

Approx. 0.013*mol0.013⋅mol

Explanation:

We need to know that 1*atm1⋅atm will support a column of mercury 760*mm760⋅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)=??*atmP=732.6⋅mm⋅Hg760⋅mm⋅Hg⋅atm−1=??⋅atm

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

n=(PV)/(RT)=((732.6*mm*Hg)/(760*mm*Hg*atm^-1)xx0.275*L)/(0.0821*L*atm*K^-1*mol^-1xx245*K)=n=PVRT=732.6⋅mm⋅Hg760⋅mm⋅Hg⋅atm−1×0.275⋅L0.0821⋅L⋅atm⋅K−1⋅mol−1×245⋅K=

1.32xx10^-2*mol.1.32×10−2⋅mol.

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

Related questions
See all questions in Ideal Gas Law
Impact of this question
1789 views around the world
You can reuse this answer
Creative Commons License