Chemical Equilibrium — Flashcards

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A reversible reaction is one that proceeds in both forward and backward directions simultaneously. It doesn't go to completion and is represented by double arrows (⇌). Example: H₂(g) + I₂(g) ⇌ 2HI(g)…

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Law of Mass Action: The rate of a chemical reaction at any instant is proportional to the product of concentration terms of all reactants. For reaction A + B → C: Rate ∝ [A][B] Rate = k[A][B] Where …

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Chemical equilibrium is the state when the rate of forward reaction equals the rate of backward reaction, and concentrations of reactants and products remain constant. Characteristics: 1. Dynamic pro…

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Equilibrium constant (Kc) is the ratio of product of concentrations of products to product of concentrations of reactants, each raised to their stoichiometric coefficients. For aA + bB ⇌ cC + dD: Kc…

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Kp is the equilibrium constant expressed in terms of partial pressures of gaseous reactants and products. For aA(g) + bB(g) ⇌ cC(g) + dD(g): Kp = (Pc)ᶜ(PD)ᵈ/(PA)ᵃ(PB)ᵇ Relationship: Kp = Kc(RT)^Δn …

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Given reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) Δn = (moles of gaseous products) - (moles of gaseous reactants) Δn = 2 - (1 + 3) = 2 - 4 = -2 Therefore: Kp = Kc(RT)⁻² Or: Kp = Kc/(RT)² Since Δn is negativ…

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Homogeneous equilibrium: All reactants and products are in the same phase. Example: H₂(g) + I₂(g) ⇌ 2HI(g) (all gases) Heterogeneous equilibrium: Reactants and products are in different phases. Examp…

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For the reaction: CaCO₃(s) ⇌ CaO(s) + CO₂(g) Kc expression: Kc = [CO₂(g)] Explanation: - Concentrations of pure solids (CaCO₃ and CaO) are constant and not included - Only gaseous and aqueous specie…