A gas occupies 0.418 litre at 740 mm of Hg and 27∘C. Calculate its Volume at STP.
Answers
1) Calculate the molecular weight:
Ideal gas law states that 1 mole of an ideal gas occupies 22.4L
therefore moles of this gas will be:
if 22.4l= 1 mole
then 0.418l = 1 x 0.418 = 0.01867 moles
22.4
moles = mass/ molecular weight
molecular weight = mass/moles
=3g/0.01867
160.69
2) New pressure if weight increases to 7.5.
Find the moles of the gas using the new mass
moles= mass/molar mass
= 7.5/160.69
= 0.0467 moles
Find volume:
If 1 mole occupies 22.4 L
then 0.0467 moles = 22.4 x 0.0467
= 1.05 liters
1.05 liters = 1050 cc
The gas initial measurements= 418 cc, 740mmHg, 27.C
resultant measurements= 1050 cc, P2, 7C(-273K)
combined gas law: P1V1/T1 =P2V2/T2
Therefore 740 x 418 = 1050 x P2
27 8
27 x 1050 x P2 = 740 x 418 x 8
28350P2 = 2474560
P2 = 2474560/28350
= 87.29 mmHg
Therefore the new pressure = 87.29 mmHg
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