On analysis, a certain compound was found to contain 254g of iodine (at.mass 127) and 80g oxygen (at.mass 16). What is the formula of the compound ?

Options

A. IO
B. `I_(2)O`
C. `I_(5)O_(3)`
D. `I_(2)O_(5)`

Answer

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

### Step 1: Calculate the moles of iodine
To find the number of moles of iodine in the compound, we use the formula:

\[ \text{Moles of Iodine} = \frac{\text{Mass of Iodine}}{\text{Molar Mass of Iodine}} \]

Given:
- Mass of iodine = 254 g
- Molar mass of iodine (I) = 127 g/mol

Calculating the moles of iodine:

\[ \text{Moles of Iodine} = \frac{254 \, \text{g}}{127 \, \text{g/mol}} = 2 \, \text{moles} \]

### Step 2: Calculate the moles of oxygen
Next, we calculate the number of moles of oxygen in the compound using the same formula:

\[ \text{Moles of Oxygen} = \frac{\text{Mass of Oxygen}}{\text{Molar Mass of Oxygen}} \]

Given:
- Mass of oxygen = 80 g
- Molar mass of oxygen (O) = 16 g/mol

Calculating the moles of oxygen:

\[ \text{Moles of Oxygen} = \frac{80 \, \text{g}}{16 \, \text{g/mol}} = 5 \, \text{moles} \]

### Step 3: Determine the simplest mole ratio
Now that we have the moles of both elements, we can find the simplest ratio of iodine to oxygen:

- Moles of iodine = 2
- Moles of oxygen = 5

The ratio of iodine to oxygen can be expressed as:

\[ \text{Ratio} = \frac{\text{Moles of I}}{\text{Moles of O}} = \frac{2}{5} \]

### Step 4: Write the empirical formula
Using the mole ratio, we can write the empirical formula of the compound. The formula will be:

\[ \text{Formula} = \text{I}_2\text{O}_5 \]

### Final Answer
The formula of the compound is **I₂O₅**.

---