On analysis ,a certain compound was found to cootains iodine and oxygen in the ratio of `254 g` of iodinite and `80 g` of oxygen .The atomic mass of oidine is `127` and the of oxygen is `16` .Which of the following is the formation of the compound ?

Options

A. IO
B. `I_(2)O`
C. `I_(5)O_(2)`
D. `I_(2)O_(5)`

Explanation

To determine the formula of the compound containing iodine and oxygen, we can follow these steps:

### Step 1: Calculate the number of moles of iodine
We know the mass of iodine is 254 g and the atomic mass of iodine is 127 g/mol.

To find the number of moles of iodine, we use the formula:
\[ \text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} \]

Substituting the values:
\[ \text{Number of moles of iodine} = \frac{254 \, \text{g}}{127 \, \text{g/mol}} = 2 \, \text{moles} \]

### Step 2: Calculate the number of moles of oxygen
The mass of oxygen is given as 80 g, and the atomic mass of oxygen is 16 g/mol.

Using the same formula:
\[ \text{Number of moles of oxygen} = \frac{80 \, \text{g}}{16 \, \text{g/mol}} = 5 \, \text{moles} \]

### Step 3: Determine the ratio of moles of iodine to moles of oxygen
From our calculations, we have:
- Moles of iodine = 2
- Moles of oxygen = 5

The ratio of moles of iodine to moles of oxygen is:
\[ \text{Ratio} = \frac{2}{5} \]

### Step 4: Write the empirical formula of the compound
Based on the ratio of moles, we can write the empirical formula of the compound as:
\[ \text{Empirical formula} = \text{I}_2\text{O}_5 \]

### Conclusion
The formula of the compound is \( \text{I}_2\text{O}_5 \).

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