Question

An oxide of nitrogen contains its half volume of nitrogen and its vapour density is 15. The molecular formula is …

Answer 1

Answer:

2

Explanation:

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