Question

12. 2074 Set B Q.No. 25 How would you apply Avogadro's hypothesis to deduce the relationship between molecular weight and vapour density of gas. An oxide of nitrogen contains half of its own volume of nitrogen and vapour density is 23. Determine its molecular formula. Ans: NO2 ​

Answer 1

Answer:

Explanation:

hey..

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n Volume of nitrogen oxides contains n / 2 volume of nitrogen . 1 volume of nitrogen oxides contains 1 / 2 volume of nitrogen .

From Avogadro Hypothesis We know that equal volume of gases at similar conditions contains same number of molecules

So we can write ,,,.

N molecules of nitrogen oxides contains n / 2 molecules of nitrogen oxides . Since nitrogen is diatomic molecules 1 / 2 molecules is equivalent to 1 atom

1 molecules of nitrogen oxides contains 1 atom of nitrogen.

We know that ,

Molecular Weight of Nitrogen = 14

Molecular Weight of Oxygen = 16

As we have 1 atom of nitrogen in one molecules of nitrogen oxides.

Vapours density of nitrogen oxides = 23

we know ,,,

Molecular Weight = vapour density *2

So Molecular Weight = 46

Let's suppose that number of Oxygen atoms be x then, 14 + x *16 = Molecular Weight

14 + 16 * x = 46

16 *X = 32

X = 2

Therefore the molecular formula of nitrogen oxides is NO2..

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hope this helps u.

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Answer 2

Explanation:

Ans No2 is the answer.

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