Convert: 5.6 liters of H2 at STP to molecules

PV = nRT?

I don't understand the qestion :p

H2 is a molecule...

... what kind of question is this?

Erm anyway I'll try my best.

5.6 Litres of H2 (like they'll give a question with a well known gas as a liquid -.-) is 0.0056m3 as a volume (which it should be at)

1 litre = 0.001m3 (or something like that)

Any gas at STP occupied 24,000cm3... SO, maybe you're trying to find the grams or the moles of gas?

wait are you on about? H2 is already a molecule (diatomic)... if you wanted it as a gas in normal volume units then what I did above is the way to go...

Thank you for posting your question to the Ask Me Help Desk.

Using the conversion factor of 1 mol H2/22.4 L H2 we can figure this out.


5.6 L H2 x 1 mol H2/22.4 L H2 x 6.02x10^23 molecules H2/1 mol H2

You should be able to solve it from here.

use the equation pv=nrt
p= pressure
v= volume
n= number of moles
r= gas constant = 8.31jk-1mol-1
t= temperature
... you have to convert the units into SI units first