NiO is to be reduced to Ni in an industrial process by the use of the reaction
`NiO(s)+CO(g) Leftrightarrow Ni(s)+CO_(2)(g)`
At 1600 K, the equilibrium constant for the reaction is 600. If a CO pressure of 150 mmHg is to be employed in the furnace and the total pressure never exceeds 760 mmHg, will the reduction occur?
(a) Yes (b) No

Answer

To determine whether the reduction of NiO to Ni will occur under the given conditions, we can use the equilibrium constant and the partial pressures of the reactants and products.

### Step-by-Step Solution:

1. **Write the Reaction and Equilibrium Expression**:
The reaction is:
\[ \text{NiO}(s) + \text{CO}(g) \leftrightarrow \text{Ni}(s) + \text{CO}_2(g) \]
The equilibrium constant \( K_p \) for this reaction is given by:
\[ K_p = \frac{P_{\text{CO}_2}}{P_{\text{CO}}} \]

2. **Given Data**:
- \( K_p = 600 \) at 1600 K
- Pressure of CO, \( P_{\text{CO}} = 150 \, \text{mmHg} \)
- Total pressure, \( P_{\text{total}} \leq 760 \, \text{mmHg} \)

3. **Calculate the Pressure of CO2**:
Since the total pressure is the sum of the partial pressures of CO and CO2, we can express it as:
\[ P_{\text{total}} = P_{\text{CO}} + P_{\text{CO}_2} \]
Rearranging gives:
\[ P_{\text{CO}_2} = P_{\text{total}} - P_{\text{CO}} \]
Substituting the maximum total pressure:
\[ P_{\text{CO}_2} = 760 \, \text{mmHg} - 150 \, \text{mmHg} = 610 \, \text{mmHg} \]

4. **Calculate the Reaction Quotient \( Q_p \)**:
Now we can calculate the reaction quotient \( Q_p \):
\[ Q_p = \frac{P_{\text{CO}_2}}{P_{\text{CO}}} = \frac{610 \, \text{mmHg}}{150 \, \text{mmHg}} \approx 4.07 \]

5. **Compare \( Q_p \) with \( K_p \)**:
We compare \( Q_p \) with \( K_p \):
- \( Q_p \approx 4.07 \)
- \( K_p = 600 \)

Since \( Q_p < K_p \), the reaction will shift to the right to reach equilibrium.

6. **Conclusion**:
Since the reaction will shift to the right, the reduction of NiO to Ni will occur under the given conditions.

### Final Answer:
(a) Yes