20 litre Nitrogen gas is poured into Jar A having a capacity of 2 litres. What will be the
volume?
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Answer:
The mole fraction of nitrogen X
N
2
=
total pressure
partial pressure ofN
2
=
5.75×10
7
torr
742.5 torr
=1.29×10
−5
55.5 moles of water are present in a liter of water. Let n be the number of moles of nitrogen. When n is small, the mole fraction of nitrogen will be X
N
2
=
n+55.5
n
=
55.5
n
Thus,
55.5
n
=1.29×10
−5
The number of moles n=55.5×1.29×10
−5
=7.16×10
−4
mol
At STP, 1 litre of a gas occupies 22.4 L or 22400 ml.
Thus the volume of nitrogen at STP =7.16×10
−4
×22400=16.0 ml.
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