The number of iodine atoms present in `1 cm^3` of its 0.1 M solution is

Options

A. `12.04 xx10^(23)`
B. `6.02xx10^(22)`
C. `12.04 xx10^(19)`
D. `6.02xx10^(20)`

Answer

To find the number of iodine atoms present in 1 cm³ of a 0.1 M iodine (I₂) solution, we can follow these steps:

### Step 1: Understand the concentration
The concentration of the solution is given as 0.1 M (molar), which means there are 0.1 moles of iodine (I₂) in 1 liter (1000 cm³) of solution.

### Step 2: Calculate the number of moles in 1 cm³
Since 1 liter = 1000 cm³, we can find the number of moles in 1 cm³ of the solution:
\[ \text{Moles in 1 cm³} = \frac{0.1 \text{ moles}}{1000 \text{ cm³}} = 0.1 \times 10^{-3} = 10^{-4} \text{ moles} \]

### Step 3: Use Avogadro's number to find the number of molecules
Avogadro's number (Nₐ) is approximately \(6.02 \times 10^{23}\) molecules/mole. To find the number of iodine molecules in 1 cm³ of the solution, we multiply the number of moles by Avogadro's number:
\[ \text{Number of I₂ molecules} = 10^{-4} \text{ moles} \times 6.02 \times 10^{23} \text{ molecules/mole} \]
\[ = 6.02 \times 10^{19} \text{ molecules} \]

### Step 4: Calculate the number of iodine atoms
Since each molecule of iodine (I₂) contains 2 iodine atoms, we need to multiply the number of molecules by 2 to find the total number of iodine atoms:
\[ \text{Number of iodine atoms} = 6.02 \times 10^{19} \text{ molecules} \times 2 \]
\[ = 12.04 \times 10^{19} \text{ atoms} \]

### Final Answer
Thus, the number of iodine atoms present in 1 cm³ of a 0.1 M iodine solution is \(12.04 \times 10^{19}\) atoms.

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