Haemoglobin contains 0.33% of iron by weight. | vedclass

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(C) Given that $100 \ g$ of haemoglobin $(Hb)$ contains $0.33 \ g$ of iron $(Fe)$.Therefore,the mass of $Fe$ in $67200 \ g$ of $Hb$ is calculated as:$

Vedclass · Accepted Answer

$4$

Vedclass · Answer

(C) Given that $100 \ g$ of haemoglobin $(Hb)$ contains $0.33 \ g$ of iron $(Fe)$.Therefore,the mass of $Fe$ in $67200 \ g$ of $Hb$ is calculated as:$	ext{Mass of } Fe = \frac{67200 	imes 0.33}{100} = 221.76 \ g$.The number of iron atoms in one molecule of haemoglobin is given by the ratio of the mass of $Fe$ in one molecule to the atomic weight of $Fe$:$	ext{Number of } Fe 	ext{ atoms} = \frac{221.76}{56} = 3.96 \approx 4$.Thus,there are $4$ iron atoms present in one molecule of haemoglobin.

Haemoglobin contains $0.33\%$ of iron by weight. The molecular weight of haemoglobin is approximately $67200$. The number of iron atoms (At. wt. of $Fe = 56$) present in one molecule of haemoglobin is

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