Question

A compound has haemoglobin like structure. It has one $Fe$. It contains $4.6\% \;$of $Fe$.Determine its molecular mass.

Answer 1

The atomic mass is the mass of a given particle: it is estimated in Dalton’s. Various atoms of a similar compound may have diverse sub-atomic masses since they contain various isotopes of a component.

Complete step by step answer:
Given : A compound has haemoglobin-like structure. It has one $Fe$. It contain $4.6\% \;$of $Fe$
Molecular weight is the mass of one molecule of a compound, while molar mass is the mass of one mole of a compound.
Molar mass is the mass of one mole of a substance. Nuclear mass is the mass of one individual unit of a substance. The nuclear mass in amu of a substance is mathematically comparable to the mass in g of one mole of that substance.
Mass of $4.6\% \;$of the compound = mass of one $Fe$ atom
Since we know, mass of one Fe atom = $55.85\,g/mol$
Therefore,
$\Rightarrow 4.6 = \dfrac{{55.85}}{{molecular\,mass\,of\,compound}} \times 100$
Hence molecular mass of the compound = $\dfrac{{55.85}}{{4.6}} \times 100$

**Hence molecular mass of the compound = $1214\,g/mol$

Note: **
Molecular weight is the mass of one molecule of a compound, while molar mass is the mass of one mole of a compound. The atomic mass is the mass of a given particle: it is estimated in Dalton’s. Various atoms of a similar compound may have diverse sub-atomic masses since they contain various isotopes of a component.