Edexcel Year 13 Chemistry: Formulas and Theorems Revision Guide | Edexcel 13年级化学：公式定理速查手册

📚 Edexcel Year 13 Chemistry: Formulas and Theorems Revision Guide | Edexcel 13年级化学：公式定理速查手册

This quick reference handbook brings together all the essential formulas, theorems and key rules from the Edexcel A Level Chemistry Year 13 syllabus. Covering reaction kinetics, equilibria, acid-base calculations, thermodynamics, electrochemistry, transition metal isomerism and organic analysis, it is designed to make last-minute revision efficient and exam-ready.

这本速查手册汇集了Edexcel A Level化学13年级大纲中所有核心的公式、定理和关键规则。内容涵盖反应动力学、平衡计算、酸碱化学、热力学、电化学、过渡金属异构现象及有机分析，旨在帮助你在考前迅速巩固要点。

1. Rate Equations & Reaction Orders | 速率方程与反应级数

rate = k[A]ᵐ[B]ⁿ

The rate equation links the speed of a reaction to the concentrations of reactants raised to their orders. The overall order of the reaction is m + n. The rate constant k is only constant at a fixed temperature and its units depend on the overall order.

速率方程将反应速率与反应物浓度的幂次联系起来，反应的总级数为 m + n。速率常数 k 仅在温度一定时恒定，其单位由总级数决定。

For a first-order reaction, the half-life is independent of initial concentration and is given by:

对于一级反应，半衰期与初始浓度无关：

t½ = ln 2 / k ≈ 0.693 / k

For a second-order reaction that depends on one reactant, the half-life depends on the initial concentration [A]₀:

对于只依赖于一种反应物的二级反应，半衰期与初始浓度 [A]₀ 相关：

t½ = 1 / (k[A]₀)

Zero-order reactions proceed at a constant rate and their concentration–time graph is a straight line with slope –k. The continuous monitoring of concentration, colorimetry or gas volume measurements can be used to track change and deduce the rate equation by the method of initial rates.

零级反应以恒定速率进行，其浓度‑时间图为一条斜率为 –k 的直线。连续监测浓度、比色法或气体体积测量均可用于追踪变化，并利用初始速率法推导速率方程。

2. Equilibrium Constants (Kc & Kp) | 平衡常数 (Kc 与 Kp)

For a homogeneous reaction aA + bB ⇌ cC + dD, the equilibrium constant in terms of concentration is:

对于均相反应 aA + bB ⇌ cC + dD，以浓度表示的平衡常数为：

Kc = ([C]ᶜ [D]ᵈ) / ([A]ᵃ [B]ᵇ)

Kc has units that depend on the stoichiometry of the reaction. Only gases and aqueous species appear; solids and pure liquids are omitted. For gas-phase equilibria, the equilibrium constant in terms of partial pressure is:

Kc 的单位取决于反应计量数，表达式中只包含气体和溶液态物种，固体与纯液体不出现在式中。对气相平衡，用分压表示的平衡常数为：

Kp = (p_Cᶜ p_Dᵈ) / (p_Aᵃ p_Bᵇ)

The partial pressure of a component is calculated from its mole fraction (x) and the total pressure P: p_i = x_i × P. The total number of moles and mole fractions must be known. Changes in temperature shift the equilibrium because the equilibrium constant itself changes with temperature; pressure changes only affect the position of equilibrium for gaseous systems with different total moles on each side, but Kp remains constant at constant temperature.

组分 i 的分压由其摩尔分数 xᵢ 与总压 P 求得：pᵢ = xᵢ × P，计算时需知道各物质的总摩尔数。温度改变会使平衡常数改变，从而移动平衡；压力改变只影响两侧气体总摩尔数不等时的平衡位置，但恒温下 Kp 保持不变。

3. Acid-Base Equilibria & pH | 酸碱平衡与 pH

Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴ mol² dm⁻⁶ (at 298 K)

The ionic product of water, Kw, links [H⁺] and [OH⁻] in any aqueous solution. At 298 K, pH + pOH = 14.00.

水的离子积 Kw 关联了任何水溶液中的 [H⁺] 与 [OH⁻]。在 298 K 时，pH + pOH = 14.00。

pH = –log₁₀[H⁺]

For a strong monoprotic acid, [H⁺] equals the acid concentration. For a weak acid HA, the acid dissociation constant Ka is used:

对强一元酸，[H⁺] 等于酸浓度。对弱酸 HA，需要用到酸的解离常数 Ka：

Ka = [H⁺][A⁻] / [HA]     pKa = –log₁₀Ka

When calculating [H⁺] of a weak acid, assume [H⁺] ≈ [A⁻] and that [HA] at equilibrium ≈ initial [HA]. Then [H⁺] ≈ √(Ka × [HA]₀).

Published by TutorHao | Year 13 Chemistry Revision Series | aleveler.com

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