A gaseous mixture was prepared by taking equal moles of CO and `N_2`. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen `(N_2)` in the mixture is

Options

A. 0.8 atm
B. 0.9 atm
C. 1 atm
D. 0.5 atm.

Explanation

To solve the problem of finding the partial pressure of nitrogen (N₂) in a gaseous mixture of equal moles of carbon monoxide (CO) and nitrogen (N₂) with a total pressure of 1 atmosphere, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Moles of CO = Moles of N₂ (equal moles)
- Total pressure (P_total) = 1 atm

2. **Understand the Concept of Partial Pressure:**
- According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture.
- Mathematically, this can be expressed as:
\[ P_{total} = P_{CO} + P_{N_2} \]

3. **Set Up the Equation:**
- Since the moles of CO and N₂ are equal, their partial pressures will also be equal. Let's denote the partial pressure of each gas as \( P \).
- Therefore, we can write:
\[ P_{CO} = P_{N_2} = P \]

4. **Substitute into the Total Pressure Equation:**
- Substitute the expressions for the partial pressures into the total pressure equation:
\[ P_{total} = P + P = 2P \]
- Since we know the total pressure is 1 atm, we can set up the equation:
\[ 1 atm = 2P \]

5. **Solve for the Partial Pressure:**
- Rearranging the equation gives:
\[ P = \frac{1 atm}{2} = 0.5 atm \]

6. **Conclusion:**
- The partial pressure of nitrogen (N₂) in the mixture is 0.5 atm.

### Final Answer:
The partial pressure of nitrogen (N₂) in the mixture is **0.5 atm**.

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