Question

Hemoglobin is the protein that transports oxygen in mammals. Hemoglobin is $\mathbf{0}\mathbf{.}\mathbf{37}\mathbf{}\mathbf{Percent}\mathbf{}\mathbf{Fe}$by mass, and each hemoglobin molecule contains four iron atoms. Calculate the molar mass of hemoglobin.

Short answer

The molar mass of hemoglobin contains four iron atoms is$6.45\times {10}^4\raisebox{1ex}{$\mathrm{g}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{mol}$}\right.$.

Step-by-step solution

Definition

Themolar mass of a material is defined asthe mass of the substance contained inone mole of the substance, and it isequal to the total massof the component atoms. It may be stated mathematically as follows:
$\mathrm{Molar}\mathrm{mass}=\frac{\mathrm{Weight}\mathrm{in}\mathrm{g}}{\mathrm{Number}\mathrm{of}\mathrm{moles}}$

Moles of F

Because the mass of iron in hemoglobin is, the mass of iron in hemoglobin may be considered to be per hemoglobin. Iron has a molecular mass of.To begin; calculate the number of moles of iron in as follows:

$\mathrm{Moles}\mathrm{of}\mathrm{Fe}=\frac{\mathrm{Mass}\mathrm{of}\mathrm{Fe}}{\mathrm{Molar}\mathrm{mass}\mathrm{of}\mathrm{Fe}}$

$$\begin{gathered} =\frac{0.347\mathrm{g}}{55.85{\displaystyle \raisebox{1ex}{$\mathrm{g}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{mol}$}\right.}} \\ =0.00621\mathrm{mol}\mathrm{Fe} \end{gathered}$$

Moles of Hemoglobin (Hb)

One mole of hemoglobin contains four moles of iron, according to the formula. So, in 0.00621 moles of iron, the number of moles of hemoglobin can be calculated as follows:

$\begin{array}{rcl}\mathrm{Moles}\mathrm{of}\mathrm{Hb}& =& \left(\frac{1\mathrm{mol}\mathrm{of}\mathrm{Hb}}{4\mathrm{mol}\mathrm{Fe}}\right)0.00621\mathrm{mol}\mathrm{Fe}\\ & =& 0.00155\mathrm{mol}\mathrm{Hb}\end{array}$

As a result, there are$0.00155$moles in of haemoglobin.

Molar mass of Hemoglobin (Hb)

The molar mass of haemoglobin may be calculated as follows:

Molar mass of Hemoglobin

$\begin{array}{rcl}\mathrm{Hb}& =& \left(\frac{\mathrm{mass}\mathrm{of}\mathrm{Hb}}{\mathrm{moles}\mathrm{of}\mathrm{Hb}}\right)\\ & =& \left(\frac{100\mathrm{g}}{0.00155\mathrm{mol}}\right)\\ & =& 64516\raisebox{1ex}{$\mathrm{g}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{mol}$}\right.\\ & =& 6.45\times {10}^4\raisebox{1ex}{$\mathrm{g}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{mol}$}\right.\end{array}$

Therefore the molar mass of Hemoglobin is$6.45\times {10}^4\raisebox{1ex}{$\mathrm{g}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{mol}$}\right.$.