For first-order: [A] = [A₀]e^(-kt) = 0.1 × e^(-0.01×100) = 0.1 × e^(-1) = 0.1 × 0.368 = 0.0368 M
For spontaneous process: ΔG < 0. Generally also ΔS > 0 for most spontaneous processes. (ΔH < 0 is not always required)
For AgCl: Ksp = [Ag⁺][Cl⁻] = s² = 1.8 × 10⁻¹⁰. s = √(1.8 × 10⁻¹⁰) = 1.34 × 10⁻⁵ mol/L
ΔG° = -nFE° = -2 × 96500 × 1.1 = -212300 J/mol = -212.3 kJ/mol
Cathode is where reduction occurs. It's the positive electrode in a galvanic cell as it attracts cations.
Using Henderson-Hasselbalch: pH = pKa + log([A⁻]/[HA]) = 4.74 + log(0.1/0.1) = 4.74
For exothermic reactions, increasing temperature decreases Kc (unfavorable) and shifts equilibrium left (Le Chatelier's principle).
i = π/(MRT) = 2.46/(0.1 × 0.0821 × 273) ≈ 1. Glucose is non-electrolyte with i = 1
Equivalent moles of strong acid and strong base neutralize completely. The salt NaCl formed doesn't hydrolyze. pH = 7
For first-order reaction: t₁/₂ = 0.693/k = 0.693/0.693 = 1 min