What is the density of neon gas given a pressure of $505mmHg$ , and a temperature of $318*K$ ?

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Answer 1 · 2017-03-14T04:00:18

We assume a litre volume of gas under these conditions.

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

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.

What is the density of neon gas given a pressure of 505*mm*Hg505*mm*Hg, and a temperature of 318*K318*K?