What is the density of neon gas given a pressure of #505*mm*Hg#, and a temperature of #318*K#?

What is the density of neon gas given a pressure of #505*mm*Hg#, and a temperature of #318*K#?

1 Answer
Mar 14, 2017

Answer:

We assume a litre volume of gas under these conditions.

And get #rho=0.5*g*L^-1#

Explanation:

Now, we know #PV=nRT#, for an Ideal Gas, and we ASSUME that neon will approximate Ideal Gas behaviour.

From the equation: #P/(RT)=n/V=("mass"/"molar mass")/V#

#P/(RT)=("mass"/"molar mass")/V=rhoxx1/"molar mass"#

And thus, (FINALLY!): #rho=P/(RT)xx"molar mass"#

And we plug in the given numbers:

#rho=((505*mm*Hg)/(760*mm*Hg*atm^-1)xx20.18*g*mol^-1)/(0.0821*(L*atm)/(K^-1*mol^-1)xx318*K)~=0.51*g*L^-1#

The units are appropriate for density, as we require. Please check my figures and assumptions; there is a lot of 'rithmetic here.