What is the density of chlorine gas at 1.21 atm and 34.9°C?

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Answer 1 · 2016-12-09T07:50:33

$rho=3.40*g*L^-1.$

We assume (reasonably) ideal gas behaviour.

And thus $PV=nRT$ , else $n/V=P/(RT)$

$=$ $(1.21*atm)/(0.0821*L*atm*K^-1*mol^-1xx307.9*K)$

$=$ $0.0479*mol*L^-1$ .

So, we have worked out a density in $mol*L^-1$ , and we multiply this by the molecular mass in $g*mol^-1$ .

And $70.9*g*mol^-1xx0.0479*mol*L^-1=3.40*g*L^-1.$

From where did I get the figure $70.9*g*mol^-1$ ?