How many grams of water vapor (H2O) are in a 10.2 liter sample at 0.98 atmospheres and 26°C? Show all work used to solve this problem.

Question

anonymous · Answer

pV=nRT,

where p-pressure, V-volume, n - amount of moles, n - gas constant (n=0.080206)

n=pV/RT

The amount of moles can be found by the equation:

n=m/M

where m - mass, M - molar mass

So the mass could be calculated as:

m=n*M

M(H2O)=18 grams/mole

 n(H2O)=0.98*10.2/0.08206*(26+273)=0.43 moles

 m(H2O)=0.43*18=7.3 grams