Haemoglobin contains `0.33%` of Fe by weight. If 1 molecule of Haemoglobin contains two Fe atoms, the molecular weight of Haemoglobin will be (at.wt of Fe = 56) nearly

Options

A. 67000
B. 34000
C. 17000
D. 20000

Explanation

To solve the problem, we need to find the molecular weight of hemoglobin based on the information given about the percentage of iron (Fe) it contains. Here’s how we can do it step by step:

### Step 1: Understand the Given Information
We know that hemoglobin contains 0.33% of iron by weight and that each molecule of hemoglobin contains two iron atoms. The atomic weight of iron (Fe) is given as 56.

### Step 2: Calculate the Total Weight of Iron in Hemoglobin
Since there are two iron atoms in one molecule of hemoglobin, the total weight of iron in one molecule can be calculated as:
\[ \text{Weight of 2 Fe atoms} = 2 \times \text{Atomic weight of Fe} = 2 \times 56 = 112 \text{ grams} \]

### Step 3: Set Up the Percentage Equation
The percentage of iron in hemoglobin is given by the formula:
\[ \text{Percentage of Fe} = \left( \frac{\text{Weight of Fe in hemoglobin}}{\text{Molecular weight of hemoglobin}} \right) \times 100 \]
We can rearrange this to find the molecular weight of hemoglobin (let's denote it as \( M \)):
\[ 0.33 = \left( \frac{112}{M} \right) \times 100 \]

### Step 4: Solve for the Molecular Weight of Hemoglobin
Now, we can solve for \( M \):
\[ 0.33 = \frac{11200}{M} \]
Multiplying both sides by \( M \):
\[ 0.33M = 11200 \]
Now, divide both sides by 0.33:
\[ M = \frac{11200}{0.33} \approx 33939.39 \text{ grams/mol} \]

### Step 5: Round Off the Molecular Weight
Since molecular weights are typically expressed in whole numbers, we can round this value:
\[ M \approx 34000 \text{ grams/mol} \]

### Final Answer
The molecular weight of hemoglobin is approximately **34000 grams/mol**.

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