If 2 moles each of CO, `N_(2)` and `CO_(2)` were taken in a 5 litre vessel at 300K and the entire `CO_(2)` was absorbed into KOH, then the partial pressure exerted by CO in the vessel after absorption will be

Options

A. 9.852 atm
B. 29.55 atm
C. 19.22 atm
D. 40 atm

Answer

To solve the problem of finding the partial pressure exerted by CO in the vessel after the absorption of CO2 by KOH, we can follow these steps:

### Step 1: Understand the Initial Conditions
We have 2 moles each of CO, N2, and CO2 in a 5-liter vessel at 300 K.

### Step 2: Determine the Total Moles Before Absorption
Initially, we have:
- Moles of CO = 2
- Moles of N2 = 2
- Moles of CO2 = 2

Total moles before absorption = 2 (CO) + 2 (N2) + 2 (CO2) = 6 moles.

### Step 3: Calculate the Partial Pressure of CO Before Absorption
Using the ideal gas law, we can calculate the partial pressure of CO before the absorption of CO2. The formula is:
\[ P = \frac{nRT}{V} \]
Where:
- \( n \) = number of moles of CO = 2
- \( R \) = ideal gas constant = 0.0821 L·atm/(K·mol)
- \( T \) = temperature in Kelvin = 300 K
- \( V \) = volume in liters = 5 L

Substituting the values:
\[ P_{CO} = \frac{2 \times 0.0821 \times 300}{5} \]

### Step 4: Perform the Calculation
Calculating the above expression:
\[ P_{CO} = \frac{49.26}{5} = 9.852 \, \text{atm} \]

### Step 5: Consider the Absorption of CO2
Since all the CO2 is absorbed by KOH, it will not contribute to the pressure in the vessel anymore. The moles of CO2 will effectively become zero.

### Step 6: Calculate the Partial Pressure of CO After Absorption
The partial pressure of CO will remain the same because the absorption of CO2 does not affect the amount of CO present in the vessel. Thus, the partial pressure of CO after the absorption of CO2 will still be:
\[ P_{CO} = 9.852 \, \text{atm} \]

### Final Answer
The partial pressure exerted by CO in the vessel after absorption will be **9.852 atm**.

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