Question

an oxide of Nitrogen contains its half volume of Nitrogen and vapour density is 23 determine the molecular weight?

Answer 1

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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Answer 2

Concept:

• Nitrogen oxides
• Ideal Gas law equation PV = nRT
• Vapour density
• The vapour density of a gas is half its molecular mass
• The density of vapour with respect to that of hydrogen is known as its vapour density.
• It can be explained as the mass of a substance in a certain volume divided by the mass of hydrogen in the same volume.

Given:

• Vapour density of the nitrogen oxide = 23

Find:

• The molecular weight of the nitrogen oxide

Solution:

We know that the molecular weight of a compound/ element is two times the value of the vapour density.

Vapour density is half the value of molecular weight.

Vapour density = 1/2 Molecular weight

Molecular weight = 2* Vapour density

Molecular weight = 2* 23 = 46

The molecular weight is 46 amu.

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