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STP chemistry problem?
What is the partial pressure of hydrogen in a flask containing 4.00 gm hydrogen and 14.0 gm nitrogen at STP? The answer should
end up as .800 atm
- Lexi RLv 71 decade agoFavorite Answer
convert each to moles
moles = mass / molar mass
moles N2 = 14.0 g / 28.02 g/mol = 0.500 moles
moles H2 = 4.00 g / 2.016 g/mol = 2.00 moles
the total pressure in a system = sum of partial pressure of each component gas
So the partial pressure is proportional to the amount of the gas in the sample.
The proportion of H2 = moles H2 / total moles
= 2.00 moles / 2.50 moles
Thus partial pressure H2 = 0.8 x total pressure
STP is standard temp (0 deg C) and pressure (1.00 atm)
partial pressure H2 = 0.8 x 1.00 atm
= 0.800 atm