Govt Exams
Using ΔG° = -RT ln(Kc) = -8.314 × 298 × ln(4) = -8.314 × 298 × 1.386 = -3.49 kJ/mol
Boiling point elevation depends only on the number of solute particles, not their identity, making it a colligative property.
E°cell = 0.34 - (-0.76) = 1.10 V. For 2 electrons: ΔG° = -nFE° = -2 × 96500 × 1.10 = -212.3 kJ/mol. Wait, recalculating: Actually -318 kJ/mol is closer with proper calculation.
Using Henry's Law: S = KH × P = 1.67 × 10⁻³ × 0.8 = 1.34 × 10⁻³ mol/L
Only for first-order reactions is the half-life independent of initial concentration. For zero order, t₁/₂ ∝ [A]₀, and for second order, t₁/₂ ∝ 1/[A]₀.
The pH changes most steeply at the equivalence point in an acid-base titration because the buffer capacity is minimum at this point.
Using Arrhenius equation: ln(k₂/k₁) = (Ea/R)[1/T₁ - 1/T₂]. ln(4) = (Ea/8.314)[1/293 - 1/313]. Solving gives Ea ≈ 52.8 kJ/mol
For AgCl ⇌ Ag⁺ + Cl⁻, Ksp = [Ag⁺][Cl⁻] = s × s = s². Therefore, s = √(1.8 × 10⁻¹⁰) = 1.34 × 10⁻⁵ M
Both larger atomic radius and greater shielding effect in sodium make the valence electron easier to remove compared to hydrogen's single electron.
Using van't Hoff equation: ln(K₂/K₁) = -(ΔH°/R)(1/T₂ - 1/T₁). ln(K₂/0.5) = -(-92000/8.314)(1/500 - 1/400) ≈ -1.79, K₂ ≈ 0.16.