A compound has hemoglobin-like structure. It has one `Fe` and contains `4.6%` of `Fe`. The approximate molecular mass is

Options

A. `1200 u`
B. `1000 u`
C. `1400 u`
D. `1600 u`

Explanation

To find the approximate molecular mass of the compound that contains 4.6% iron (Fe) and has a hemoglobin-like structure, we can follow these steps:

### Step 1: Understand the relationship between percentage composition and molecular mass
The percentage of an element in a compound is given by the formula:
\[ \text{Percentage of element} = \left( \frac{\text{mass of element per mole}}{\text{molecular mass of compound}} \right) \times 100 \]
In this case, the element is iron (Fe).

### Step 2: Identify the mass of iron
The molar mass of iron (Fe) is approximately 56 g/mol. Since the compound contains 1 atom of Fe, the mass of Fe per mole in the compound is 56 g.

### Step 3: Set up the equation using the given percentage
We know that the percentage of Fe in the compound is 4.6%. We can set up the equation as follows:
\[ 4.6 = \left( \frac{56}{\text{molecular mass of compound}} \right) \times 100 \]

### Step 4: Rearrange the equation to solve for the molecular mass of the compound
Rearranging the equation gives us:
\[ \text{molecular mass of compound} = \frac{56 \times 100}{4.6} \]

### Step 5: Calculate the molecular mass
Now, we can calculate the molecular mass:
\[ \text{molecular mass of compound} = \frac{5600}{4.6} \approx 1217.39 \text{ g/mol} \]

### Step 6: Round to the nearest whole number
The approximate molecular mass is about 1217 g/mol. If we check the options provided, the nearest option would be 1200 g/mol.

### Final Answer
The approximate molecular mass of the compound is **1200 g/mol**.