divided the mole value obtained above by the smallest number.
Answers
Explanation:
Step 1 : Conversion of the mass percent to grams.
Since we are having the mass percent, it is convenient to use 100 g of the compound as the starting material. Thus, in the 100 g sample of the above compound, 12.5 g of hydrogen is present and 87.5 g of nitrogen is present.
Step 2 : Convert into number moles of each element
Divide the masses obtained above by respective atomic masses of various elements.
Moles of Hydrogen =
1
12.5
=12.5
Moles of Nitrogen =
14
87.5
=6.25
Step 3 : Divide the mole value obtained above by the smallest number.
Since 6.25, is the smallest value, division by it gives a ratio of 2:1 for H:N.
Step 4 : Write empirical formula by mentioning the numbers after writing the symbols of the respective elements.
NH
2
is thus the empirical formula of the above compound.
Step 5 : Writing molecular formula.
(a) Determine empirical formula mass. Add the atomic masses of various atoms present in the empirical formula.
For NH
2
, empirical formula mass is 14+2=16 g.
(b) Divide Molar mass by empirical formula mass
Molecular weight=2×vapour density=2×16=32
Empiricalweight
Molarweight
=2=n
(c) Multiply empirical formula by n obtained above to get the molecular formula
Molecular formula −
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