The molar volume of CO2 at 0 degree and 2.0.atm is :

Explanation

To find the molar volume of CO2 at 0 degrees Celsius and 2.0 atm, we can use the Ideal Gas Law, which is represented by the equation:

\[ PV = nRT \]

Where:
- \( P \) = pressure
- \( V \) = volume
- \( n \) = number of moles
- \( R \) = ideal gas constant
- \( T \) = temperature in Kelvin

### Step 1: Convert Temperature to Kelvin
The temperature given is 0 degrees Celsius. To convert this to Kelvin, we use the formula:

\[ T(K) = T(°C) + 273.15 \]

So,

\[ T = 0 + 273.15 = 273.15 \, K \]

### Step 2: Identify the Values
From the question, we have:
- Pressure \( P = 2.0 \, atm \)
- Number of moles \( n = 1 \, mole \) (since we are calculating the molar volume)
- Ideal gas constant \( R = 0.0821 \, L \cdot atm/(K \cdot mol) \)

### Step 3: Rearrange the Ideal Gas Law for Volume
We can rearrange the Ideal Gas Law to solve for volume \( V \):

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

### Step 4: Substitute the Values into the Equation
Now we can substitute the values we have into the equation:

\[ V = \frac{(1 \, mol) \times (0.0821 \, L \cdot atm/(K \cdot mol)) \times (273.15 \, K)}{2.0 \, atm} \]

### Step 5: Calculate the Volume
Now, we perform the calculation:

1. Calculate the numerator:
\[ 1 \times 0.0821 \times 273.15 = 22.414 \, L \cdot atm \]

2. Divide by the pressure:
\[ V = \frac{22.414}{2.0} = 11.207 \, L \]

### Step 6: Round the Result
Rounding the result gives us:

\[ V \approx 11.2 \, L \]

### Conclusion
The molar volume of CO2 at 0 degrees Celsius and 2.0 atm is approximately **11.2 liters**.

---