Indicate whether ΔG increases, decreases, or stays the same for each of the following reactions as the partial pressure of O₂ is increased: (a) 2 CO(g) + O₂(g) → 2 CO₂(g) (b) 2 H₂O₂(l) → 2 H₂O(l) + O₂(g) (c) 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Verified step by step guidance

1. Step 1: Understand the relationship between Gibbs free energy change (ΔG) and reaction quotient (Q). The equation ΔG = ΔG° + RT ln(Q) shows that ΔG depends on the reaction quotient Q, which is affected by the partial pressures of gases involved in the reaction.
2. Step 2: For reaction (a) 2 CO(g) + O₂(g) → 2 CO₂(g), increasing the partial pressure of O₂ will decrease Q because O₂ is a reactant. Since Q decreases, ln(Q) becomes more negative, which decreases ΔG, making the reaction more spontaneous.
3. Step 3: For reaction (b) 2 H₂O₂(l) → 2 H₂O(l) + O₂(g), increasing the partial pressure of O₂ will increase Q because O₂ is a product. Since Q increases, ln(Q) becomes more positive, which increases ΔG, making the reaction less spontaneous.
4. Step 4: For reaction (c) 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g), increasing the partial pressure of O₂ will increase Q because O₂ is a product. Since Q increases, ln(Q) becomes more positive, which increases ΔG, making the reaction less spontaneous.
5. Step 5: Summarize the effects: (a) ΔG decreases, (b) ΔG increases, (c) ΔG increases, as the partial pressure of O₂ is increased.