Equilibrium

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Dynamic equilibrium is a state where the rate of forward reaction equals the rate of reverse reaction, with no net change in concentration of reactants and products. Unlike static equilibrium where th

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Kc = [NH₃]²/([N₂][H₂]³) For the general reaction aA + bB ⇌ cC + dD: Kc = [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ Products in numerator, reactants in denominator, each raised to their stoichiometric coefficients.

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Kp = Kc(RT)^Δn Where: - Δn = (moles of gaseous products) - (moles of gaseous reactants) - R = 0.0831 bar L mol⁻¹ K⁻¹ - T = temperature in Kelvin Derivation: Since p = [gas]RT for each gas, substitut

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Reaction quotient (Q) has the same expression as K but uses concentrations at any time, not just at equilibrium. Predicting direction: - If Q < K: reaction proceeds forward (→) - If Q > K: reaction p

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Le Chatelier's Principle: When a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will shift to counteract the applied change. Example: For N₂ + 3

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Temperature is the ONLY factor that changes the value of K: Exothermic reactions (ΔH < 0): - Increasing temperature → K decreases - Decreasing temperature → K increases Endothermic reactions (ΔH > 0

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Arrhenius: - Acid: produces H⁺ in water - Base: produces OH⁻ in water Brönsted-Lowry: - Acid: proton (H⁺) donor - Base: proton (H⁺) acceptor Lewis: - Acid: electron pair acceptor - Base: electron pa

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A conjugate acid-base pair differs by only one proton (H⁺). Conjugate acid = base + H⁺ Conjugate base = acid - H⁺ Examples: - HCl/Cl⁻ (HCl is acid, Cl⁻ is conjugate base) - NH₃/NH₄⁺ (NH₃ is base, NH