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For the reaction: X₂O₄(l) → 2XO₂(g) ΔU = -2.1 kcal, ΔS = 20 cal K⁻¹ at 300 K. Hence ΔG is:

1. -2.7 kcal
2. -2.7 k cal
3. 9.3 k cal
4. -9.3 k cal

Correct answer: -2.7 kcal

Solution

The Gibbs free energy change (ΔG) is calculated using the formula ΔG = ΔU - TΔS. Substituting the given values: ΔU = -2.1 kcal, T = 300 K, and ΔS = 20 cal K⁻¹ (convert to kcal: 20/1000 = 0.02 kcal K⁻¹), we get ΔG = -2.1 - (300 × 0.02) = -2.1 - 6 = -2.7 kcal.

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