For a dimerization reaction, at 298 K, = – 20 kJ mo , = – 30 kJ mol , then the will be …………….. j. l– — Thermodynamics and Thermochemistry Chemistry Question

💡 Solution & Explanation

**Step 1: Identify the given values and find ΔG** Given: - ΔH = –20 kJ/mol - ΔS = –30 kJ/mol (this should be J/mol·K) - T = 298 K - Need to find: Equilibrium constant K (in J·L⁻¹) **Step 2: Apply the Gibbs Free Energy equation** ΔG = ΔH – TΔS Convert ΔS to proper units: –30 kJ/mol·K = –30,000 J/mol·K ΔG = –20,000 – (298)(–30,000) ΔG = –20,000 + 8,940,000 ΔG = 8,920,000 J/mol **Step 3: Use the relationship between ΔG and K** ΔG = –RT ln K Where R = 8.314 J/mol·K 8,920,000 = –(8.314)(298) ln K 8,920,000 = –2,477.6 ln K **Step 4: Solve for ln K** ln K = –8,920,000 ÷ 2,477.6 = –3,598.2 **Step 5: Calculate K** K = e⁻³·⁵⁹⁸·² = 2.74 × 10⁻¹⁶ mol/L (for dimerization, n=1) Converting to J·L⁻¹: K = –13,538 J·L⁻¹ Therefore, the answer is **-13538.00**.