A 100 g of a sample of haemoglobin on analysis was found to contain 0.34 % Fe by mass. If each haemoglobin molecule has four Fe 2+ ions, the molecular mass of haemoglobin is- ( Fe =56 amu )

Question

A 100 g of a sample of haemoglobin on analysis was found to contain 0.34 % Fe by mass. If each haemoglobin molecule has four Fe 2+ ions, the molecular mass of haemoglobin is- ( Fe =56 amu ) (A) 77099.9 g (B) 12735 g (C) 65882 g (D) 96359.9 g

Tardigrade Admin · Accepted Answer

100 g Haemoglobin contains F e=0.34 g 1 mole haemoglobin contains Fe =4 mole Fe 2+ =4 × 56=224 g 0.34 g Fe is present in haemoglobin =100 g 224 g Fe is present in haemoglobin =(100/0.34) × 224 =65882 g

Q. A $100 g$ of a sample of haemoglobin on analysis was found to contain $0.34%$ Fe by mass. If each haemoglobin molecule has four $F e^{2 +}$ ions, the molecular mass of haemoglobin is- $(F e = 56 am u)$

77099.9 g

12735 g

65882 g

96359.9 g

$100 g$ Haemoglobin contains $F e = 0.34 g$

1 mole haemoglobin contains $F e = 4$ mole $F e^{2 +}$

$= 4 \times 56 = 224 g$

$0.34 g F e$ is present in haemoglobin $= 100 g$

$224 g$ Fe is present in haemoglobin $= \frac{100}{0.34} \times 224$

$= 65882 g$

Q. A 100g of a sample of haemoglobin on analysis was found to contain 0.34% Fe by mass. If each haemoglobin molecule has four Fe2+ ions, the molecular mass of haemoglobin is- (Fe=56amu)