Consider this reaction at equilibrium: 2KClO3(s) ⇌ 2KCl(s) + 3O2(g). Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. O2 is removed from the reaction mixture. b. KCl is added to the reaction mixture. c. KClO3 is added to the reaction mixture. d. O2 is added to the reaction mixture.

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1. Identify the principle governing the reaction shifts: Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
2. For part (a), removing O2 decreases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the right to produce more O2.
3. For part (b), adding KCl increases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the left to reduce the concentration of KCl.
4. For part (c), adding KClO3 increases the concentration of a reactant. Since KClO3 is a solid, its concentration does not affect the equilibrium position, so the equilibrium remains unchanged.
5. For part (d), adding O2 increases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the left to reduce the concentration of O2.