Question

A molecule has two nitrogen and four hydrogen atoms if the symbols of nitrogen and hydrogen are
N and respectively then write its empirical formula and determine its molar maso

Answer 1

Answer:





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Question



A gaseous compound of nitrogen and hydrogen contains 12.5 % hydrogen by mass. The molecular formula of the compound if its relative molecular mass is 32, is:  [N=14, H=1] 

A

NH4

B

N2H3

C

N2H6

D

N2H4

Correct Answer

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Solution



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Correct option is D)

100 g of the compound contains 12.5 g H and 100−12.5=87.5 g N.

The atomic masses of H and N are 1 g/mol and 14 g/mol respectively.

The number of moles of H =1 g/mol  12.5 g= 12.5 mol 

The number of moles of N =14 g/mol  87.5 g= 6.25 mol 

The mole ratio N:H=6.25:12.5=1:2

Hence, the empirical formula of the compound is NH2.

Molecular formula  =(NH2)× empirical formula weight Molecular weight 

Molecular formula  =(NH2)× 16 g/mol 32 g/mol 

The molecular formula of the compound is N2H4.

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Answer 2

Explanation:

A molecule has two nitrogen and four hydrogen atoms.

When nitrogen reacts with hydrogen ammonium.

\dispalystyle \mathbf {2N2(g) + 4H2(g) \rightarrow 2NH4(g)}\dispalystyle2N2(g)+4H2(g)→2NH4(g)

∴ Its empirical formula is \dispalystyle \mathbf {NH4}\dispalystyleNH4

Molar mass of Hydrohen is 1.00794 g/mol

Molar mass of Nitrogen is 14.0067 g/mol

∴ Molar mass = 1*N + 4*H

= 1*( 1.00794 ) + 4*( 14.0067 )

= 1.00794 + 56.0268

M = 57.03474 g/mo