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Using the Gibbs energy change, ΔG° = −63.3 kJ, for the following reaction, Ag2CO3 → 2Ag⁺ (aq) + CO3²⁻ (aq), the Ksp of Ag2CO3(s) in water at 25°C is: (R = 8.314 J K⁻¹ mol⁻¹)

1. 3.2 × 10⁻²⁶
2. 8.0 × 10⁻¹²
3. 2.9 × 10⁻³
4. 7.9 × 10⁻²

Correct answer: 8.0 × 10⁻¹²

Solution

The relationship between ΔG° and Ksp is given by ΔG° = -RT ln(Ksp). Substituting ΔG° = -63.3 kJ = -63300 J, R = 8.314 J K⁻¹ mol⁻¹, and T = 298 K, we solve for Ksp: ln(Ksp) = ΔG° / (-RT). This gives Ksp ≈ 8.0 × 10⁻¹².

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