Verified Answer :
Answer:N2H4
Explanation: Empirical Formula, EF= NH2
Mass of the EF = mass of Nitrogen + mass of Hydrogen
EF = 14.007 + 1.008
= 15.015
Then, divide the given formula mass by the EF. That is,
32.06/15.015 = 2.135 = 2 (to the nearest whole number) ......... (1)
To get the molecular formula, multiple the empirical formula with the number from the equ (1) above.
Molecular formula = 2[NH2] = N2H4
The empirical formula is defined as the simplest whole-number ratio of atoms present in a compound. A molecular formula determines the number of atoms present in each element of the compound.
The molecular formula of a given compound is \(\rm N_2H_4\).
Given:
- Empirical formula = \(\rm NH_2\)
- Mass of \(\rm NH_2\) = mass of Nitrogen + mass of hydrogen = 15.01
- Formula mass of \(\rm NH_2\) = 32.0 amu
To find the molecular formula, we get:
Molecular formula = \(\dfrac{32.06}{2.135}\) = 2 (nearest whole number)
Multiplying the empirical formula with the value of the molecular formula obtained above, we get:
Molecular formula:
\(2 \times \rm NH_2\) = \(\rm N_2H_4\)
Thus, the molecular formula of a given compound is \(\rm N_2H_4\).
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