The osmotic pressure of a solution containing 0.1 mol of solute per litre at 323 K is

Answer

To calculate the osmotic pressure of a solution, we can use the formula:

\[ \pi = \frac{n}{V} \cdot R \cdot T \]

where:
- \(\pi\) = osmotic pressure
- \(n\) = number of moles of solute
- \(V\) = volume of the solution in liters
- \(R\) = universal gas constant (0.0821 atm·L/(mol·K))
- \(T\) = temperature in Kelvin

### Step-by-Step Solution:

1. **Identify the given values:**
- Number of moles of solute (\(n\)) = 0.1 mol
- Volume of the solution (\(V\)) = 1 L (since it is given as per liter)
- Temperature (\(T\)) = 323 K
- Universal gas constant (\(R\)) = 0.0821 atm·L/(mol·K)

2. **Substitute the values into the formula:**
\[ \pi = \frac{0.1 \, \text{mol}}{1 \, \text{L}} \cdot 0.0821 \, \text{atm·L/(mol·K)} \cdot 323 \, \text{K} \]

3. **Calculate the osmotic pressure:**
\[ \pi = 0.1 \cdot 0.0821 \cdot 323 \]

4. **Perform the multiplication:**
\[ \pi = 0.1 \cdot 26.5253 \approx 2.65253 \, \text{atm} \]

5. **Final result:**
\[ \pi \approx 2.65 \, \text{atm} \]

### Final Answer:
The osmotic pressure of the solution is approximately **2.65 atm**.