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Question

A, B and C are three cylinders of volume 11.2 L each. H2,O2 and N2 gases at STP are filled in A, B and C respectively.
(a) Find the number of moles of H2 molecules in A.
(b) Calculate the number of molecules of O2 present in B.(c)IfthevolumeofN,presentinCisdoubledatSTP,calculatethemassingramofN_2gas.[given:MolarvolumeatSTP= 22.4L,At.mass:H = 1,\ O= 16,\ N = 14$]

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Solution

The volume of one mole of any gas at STP is 22.4 L and there are 6.022×1023 molecules in it.
(a) The volume of H2 at STP in cylinder A is 11.2 L
The number of moles in 11.2 L =11.222.4=0.5
The number of H2 molecules =0.5×6.022×1023
(b) The number of moles of O2 molecules in 11.2 L =0.5×6.022×1023=3.011×1023
(c) The number of moles of N2 in 11.2 L =11.222.4=0.5
Mass of 1 mole of N2=28g
Mass of 0.5 moles of N2=14g
If the volume of N2 at STP is doubled, it becomes 22.4 L. It means 1 mole of N2.
Therefore, the mass of N2 in grams when the volume is 22.4 L is 28 g.

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