Mass % Iron:

$\mathbf{\%}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{}\mathbf{in}\mathbf{}\mathbf{hemoglobin}}{\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{hemoglobin}}\mathbf{\times}\mathbf{100}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{hemoglobin}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{}\mathbf{in}\mathbf{}\mathbf{hemoglobin}}{{\displaystyle \frac{\mathbf{\%}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{Fe}}{\mathbf{100}}}}$

- MW of Fe = 55.85 g/mol

Hemoglobin, the oxygen-carrying protein in red blood cells, has four iron atoms per molecule and contains 0.340% iron by mass. Calculate the molar mass of hemoglobin. Express your answer using three significant figures.

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