At STP, what will be the volume of `6.022 xx 10^(23)` molecules of `H_(2)` ?

Answer

To find the volume of \(6.022 \times 10^{23}\) molecules of \(H_2\) at standard temperature and pressure (STP), we can follow these steps:

### Step 1: Understand the relationship between moles and molecules
We know that 1 mole of any substance contains \(6.022 \times 10^{23}\) molecules. This number is known as Avogadro's number.

### Step 2: Determine the number of moles
Since the question provides \(6.022 \times 10^{23}\) molecules of \(H_2\), we can determine that this is equivalent to 1 mole of hydrogen gas.

\[ \text{Number of moles} = \frac{\text{Number of molecules}}{6.022 \times 10^{23}} = \frac{6.022 \times 10^{23}}{6.022 \times 10^{23}} = 1 \text{ mole} \]

### Step 3: Use the volume of 1 mole at STP
At STP, 1 mole of any ideal gas occupies a volume of 22.4 liters. Therefore, since we have 1 mole of \(H_2\):

\[ \text{Volume at STP} = 1 \text{ mole} \times 22.4 \text{ L/mole} = 22.4 \text{ liters} \]

### Final Answer
Thus, the volume of \(6.022 \times 10^{23}\) molecules of \(H_2\) at STP is **22.4 liters**.

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