What is the density of hydrogen gas using the ideal gas law?

Answer 1

Of course, for #"density"# we need to SPECIFY....#"temperature"# and #"pressure...."#

And, using standard conditions of #P=1*atm#...and #T=298*K#, we address the Ideal Gas equation...(at least near standard conditions....)

#PV=nRT#...#n/V=P/(RT)=("mass"/"molar mass")/V=P/(RT)#

And thus...

#underbrace("mass"/V)_("density"=rho)=P/(RT)xx"molar mass"#

And thus our working equation...#rho_(H_2)=P/(RT)xx2.016*g*mol^-1#

#=(1*atmxx2.016*g*mol^-1)/(0.0821*(L*atm)/(K*mol)xx298*K)~=0.1*g*L^-1#

We note that hydrogen gas, as are all elemental gases with any chemistry, is bimolecular, i.e. #H_2#...

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Answer 2

Owen Ambrose

The density of hydrogen gas using the ideal gas law is approximately 0.0899 grams per liter at standard temperature and pressure (STP).

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.