A given sample of phosphorus contains 0.25 mol of phosphorus molecules (`P_4`). The number of moles of phosphorus atoms, number of phosphorus molecules and number of phosphorus atoms present in the given sample are respectively

Options

A. `6.023xx10^24 , 1` and `3.2xx10^23`
B. `4 , 3.2 xx 10^23` and `6.023xx10^24`
C. `1,1.5xx10^23` and `6.023xx10^23`
D. `6.023xx10^24 , 3.2 xx 10^23` and 2

Answer

To solve the problem, we need to determine the number of moles of phosphorus atoms, the number of phosphorus molecules, and the total number of phosphorus atoms present in a sample that contains 0.25 moles of phosphorus molecules (P₄).

### Step-by-Step Solution:

1. **Identify the number of moles of phosphorus molecules:**
- The problem states that we have 0.25 moles of phosphorus molecules (P₄).

2. **Calculate the number of moles of phosphorus atoms:**
- Each molecule of P₄ contains 4 phosphorus atoms.
- Therefore, to find the number of moles of phosphorus atoms, we multiply the number of moles of P₄ by 4:
\[ \text{Moles of phosphorus atoms} = 0.25 \, \text{moles of P₄} \times 4 \, \text{atoms/molecule} = 1.0 \, \text{moles of phosphorus atoms} \]

3. **Determine the number of phosphorus molecules:**
- The number of phosphorus molecules is given directly as 0.25 moles of P₄.

4. **Calculate the total number of phosphorus atoms:**
- To find the total number of phosphorus atoms, we use Avogadro's number (approximately \(6.022 \times 10^{23}\) atoms/mole).
- First, we calculate the number of phosphorus atoms:
\[ \text{Total number of phosphorus atoms} = \text{Moles of phosphorus atoms} \times \text{Avogadro's number} \]
\[ = 1.0 \, \text{moles} \times 6.022 \times 10^{23} \, \text{atoms/mole} = 6.022 \times 10^{23} \, \text{atoms} \]

### Final Results:
- Number of moles of phosphorus atoms: **1.0 moles**
- Number of phosphorus molecules: **0.25 moles**
- Total number of phosphorus atoms: **\(6.022 \times 10^{23}\) atoms**