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For the equilibrium reaction BaO2(s) ⇌ BaO(s) + O2(g), where ΔH is positive, the equilibrium constant Kp is expressed in terms of the partial pressure of O2. Given that the reaction is endothermic, an increase in temperature favors the production of O2.

1. Kp equals the partial pressure of O2.
2. Kp is the reciprocal of the partial pressure of O2.
3. Kp is proportional to the square of the partial pressure of O2.
4. None of the above is correct.

Correct answer: Kp equals the partial pressure of O2.

Solution

The equilibrium constant Kp is defined as the partial pressure of O2 (PO2) for this reaction because only O2 is in the gaseous state, and the reaction involves its formation. Since ΔH is positive, increasing temperature favors the formation of O2, consistent with Le Chatelier's principle.

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