Final answer:
The question is asking for the partial pressure of oxygen (PO₂) at equilibrium for a specific reaction, but lacks the necessary partial pressure of nitrogen dioxide (PNO₂) to complete the calculation.
Step-by-step explanation:
The student is asking to calculate the equilibrium partial pressure of oxygen (PO₂) for the reaction 2NO₂(g) ⇌ 2NO(g) + O₂(g) given that the equilibrium constant Kp is 158 at 1000 K, the partial pressure of nitrogen dioxide (PNO₂) is unknown, and the partial pressure of nitric oxide (PNO) is 0.270 atm. To solve this problem, we need to use the equation for the equilibrium constant in terms of partial pressures (Kp) which is expressed as:
Kp = (PNO)^2 * (PO₂) / (PNO₂)^2
Since we are given Kp and PNO, but not PNO₂, we cannot directly calculate PO₂. The question seems incomplete as it lacks the value of PNO₂ required to proceed with the calculations.