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### Given Information:
- **Mass of Mg (Magnesium):** 22.3 g
- **Atomic mass of Mg:** 24.31 g/mol
- **Temperature (T):** 300 K
- **Pressure (P):** 1 atm
- **Ideal gas constant (R):** 0.08205 L·atm/(mol·K)

### Step 1: Determine the moles of Mg.
From the chemical equation:

\[
\text{Mg} + 2 \text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2
\]

1 mole of Mg produces 1 mole of \( \text{H}_2 \). First, we calculate the number of moles of Mg:

\[
n(\text{Mg}) = \frac{\text{mass of Mg}}{\text{molar mass of Mg}} = \frac{22.3 \, \text{g}}{24.31 \, \text{g/mol}} = 0.917 \, \text{mol}
\]

Since the molar ratio of Mg to \( \text{H}_2 \) is 1:1, the number of moles of \( \text{H}_2 \) produced is also 0.917 mol.

### Step 2: Use the Ideal Gas Law to find the volume of \( \text{H}_2 \).

The ideal gas law is:

\[
PV = nRT
\]

Rearranging for \( V \):

\[
V = \frac{nRT}{P}
\]

Substitute the known values:

\[
V = \frac{(0.917 \, \text{mol}) \times (0.08205 \, \text{L·atm/mol·K}) \times (300 \, \text{K})}{1 \, \text{atm}} 
\]

\[
V = \frac{(0.917) \times (0.08205) \times (300)}{1} = 22.55 \, \text{L}
\]

So, the volume of hydrogen gas (\( \text{H}_2 \)) produced is approximately **22.55 liters**.

### Final Answer: 
The volume of \( \text{H}_2 \) released is approximately **22.55 L**.

Would you like to go into more detail on any step? Feel free to ask!

Here are 5 related questions:
1. How would the result change if the pressure was doubled to 2 atm?
2. What would happen if we had 30 g of Mg instead of 22.3 g?
3. How does the ideal gas law change if the temperature is halved?
4. Can the ideal gas law be used for gases at very high pressures?
5. How would the result differ if the gas were collected at 400 K instead of 300 K?

**Tip:** Always check your units carefully when using the ideal gas law to ensure the correct gas constant (R) value.

What volume of H2 is released when 22.3 g of Mg reacts completely with HCl at a temperature of 300 K and a pressure of 1 atm?

Solve this Ideal Gas Law problem where 22.3 g of Mg reacts with HCl at 300 K and 1 atm to release H2. Learn step-by-step calculations, including stoichiometry and gas laws. Suitable for high school students in Grades 10-12.

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