Answer:
The reaction will proceed in the forward direction, resulting in the reduction of NiO to Ni
Explanation:
Step 1: Provided data
Kp = 6.0 * 10²
Pressure of CO = 150 torr
Total pressure remains under 760 torr
Step 2: The balanced reaction equation:
NiO(s) + CO(g) ⇆ Ni(s) + CO2(g)
Step 3: Determine P(CO) and P(CO2)
For this equilibrium, the Kp expression is:
Kp = P(CO2)/P(CO) = 6.0*10^2
Given that NiO and Ni are solids, they do not affect the Kp
⇒ with P(CO) = 150 torr
⇒ P(CO) = 760 - 150 = 610 torr
Step 4: Calculate the reaction quotient
Q = 610/150 = 4.1
Since Q is significantly less than Kp, there are more reactants than products. Some reactants will convert into products, driving the reaction rightward.
Thus, the reaction will proceed forward, leading to the reduction of NiO to Ni.
