The total concentration of dissolved particles in side red blood cells is approximately `0.30 M` and the membrane surrounding the cells is semipermeable. What would be the atmosheric pressure in atm inside the cells become if the cells were removed from blood plasma and placed in pure water at `298 K`. Also what would happen to red blood cells?

Options

A. `7.34` atm
B. `1.78` atm
C. `2.34` atm
D. `0.74` atm

Explanation

To solve the problem, we need to calculate the osmotic pressure of the red blood cells when they are placed in pure water. We will use the formula for osmotic pressure, which is given by:

\[ \pi = CRT \]

Where:
- \(\pi\) = osmotic pressure
- \(C\) = concentration of the solution (in molarity)
- \(R\) = ideal gas constant (0.0821 L·atm/(K·mol))
- \(T\) = temperature in Kelvin

### Step 1: Identify the given values
- Concentration (\(C\)) = 0.30 M
- Temperature (\(T\)) = 298 K
- Ideal gas constant (\(R\)) = 0.0821 L·atm/(K·mol)

### Step 2: Substitute the values into the osmotic pressure formula
\[ \pi = (0.30 \, \text{mol/L}) \times (0.0821 \, \text{L·atm/(K·mol)}) \times (298 \, \text{K}) \]

### Step 3: Calculate the osmotic pressure
\[ \pi = 0.30 \times 0.0821 \times 298 \]
\[ \pi = 0.30 \times 24.4758 \approx 7.34 \, \text{atm} \]

### Conclusion:
The osmotic pressure inside the cells would be approximately **7.34 atm**.

### Step 4: Determine what happens to red blood cells
When red blood cells are placed in pure water, which is a hypotonic solution compared to the blood plasma, water will move into the cells due to osmosis. This will cause the cells to swell and potentially burst.

### Final Answer:
1. The osmotic pressure inside the cells would become **7.34 atm**.
2. The red blood cells would swell and may burst due to the influx of water.

---