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The problem shown in the image is asking for the pressure that 10 grams of molecular hydrogen (H₂) would exert at a temperature of 300°C and a volume of 80 liters.

The solution provided follows these steps:

### Step 1: Calculate the moles of hydrogen (H₂)

To find the number of moles (\(n\)) of hydrogen gas, we use the relation:

\[
n = \frac{\text{mass}}{\text{molar mass}}
\]

Given:
- Mass of H₂ = 10 grams
- Molar mass of H₂ = 2.02 grams/mol

\[
n = \frac{10 \, g}{2.02 \, g/mol} = 4.95 \, \text{moles of H₂}
\]

### Step 2: Convert temperature to Kelvin

The temperature is provided in degrees Celsius (300°C). To convert it to Kelvin:

\[
T = 300^\circ C + 273 = 573 \, K
\]

### Step 3: Convert volume to cubic meters

The volume is given in liters (80 L), and we convert it to cubic meters (m³):

\[
V = 80 \, L \times \frac{1 \, m³}{1000 \, L} = 0.08 \, m³
\]

### Step 4: Use the ideal gas law

The ideal gas law is:

\[
pV = nRT
\]

Where:
- \(p\) is the pressure (Pa)
- \(V\) is the volume (m³)
- \(n\) is the number of moles (mol)
- \(R\) is the ideal gas constant \(8.31 \, \text{J/mol·K}\)
- \(T\) is the temperature in Kelvin

Plugging in the values:

\[
p \times 0.08 = 4.95 \times 8.31 \times 573
\]

Solving for pressure \(p\):

\[
p = \frac{4.95 \times 8.31 \times 573}{0.08}
\]

\[
p \approx 2.95 \times 10^5 \, \text{Pa}
\]

So, the pressure is approximately \(2.95 \times 10^5\) Pascals (Pa), or 295 kPa.

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Would you like more details on any of the steps? Here are some related questions you might consider:

1. How does the ideal gas law relate to real gas behavior?
2. Why do we need to convert temperature to Kelvin in gas law calculations?
3. How does molecular weight affect the number of moles of a substance?
4. How does pressure change with increasing volume under constant temperature and moles?
5. Can the ideal gas law be applied to liquids?

**Tip:** Always convert all quantities to SI units when using the ideal gas law to avoid calculation errors.

Quina pressió exercirà 10 g d’hidrogen molecular si està a 300 ºC i ocupa un volum de 80 L?

Find the pressure exerted by 10 grams of molecular hydrogen (H₂) at a temperature of 300°C and a volume of 80 liters using the ideal gas law. The problem involves unit conversions, the calculation of moles of H₂, and application of the ideal gas law formula. Suitable for Grades 10-12.

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