📚 IB Edexcel Chemistry: Formula Summary Handbook | IB与爱德思化学公式汇总手册
Mastering the essential formulas is crucial for success in IB and Edexcel A-Level Chemistry. This handbook provides a concise yet comprehensive collection of the most important equations you will encounter across topics such as stoichiometry, energetics, kinetics, equilibrium, acids and bases, thermodynamics, electrochemistry, and organic quantitative chemistry. Each section pairs clear English explanations with Chinese translations to reinforce understanding.
掌握核心公式是IB和爱德思A-Level化学成功的关键。本手册精选了化学计量学、热力学、动力学、平衡、酸碱、热力学、电化学和有机定量化学等主题中最关键的方程式。每个部分都以清晰的中英文对照解释，帮助加深理解。
1. The Mole and Stoichiometric Calculations | 摩尔与化学计量计算
The mole connects the macroscopic world to the particulate level. The amount of substance n can be found from mass, solution volume, or gas volume.
摩尔将宏观世界与微粒水平联系起来。物质的量 n 可从质量、溶液体积或气体体积求得。
n = m / M (mass m in g, molar mass M in g mol⁻¹)
n = m / M (质量 m 单位 g，摩尔质量 M 单位 g mol⁻¹)
n = c × V (c in mol dm⁻³, V in dm³)
n = c × V (c 单位 mol dm⁻³，V 单位 dm³)
n = V(gas) / Vₘ (Vₘ = 22.7 dm³ mol⁻¹ at STP for IB, 24 dm³ mol⁻¹ at RTP for Edexcel)
n = V(气体) / Vₘ (IB 标准状况 Vₘ = 22.7 dm³ mol⁻¹，爱德思常温常压 Vₘ ≈ 24 dm³ mol⁻¹)
Number of particles: N = n × L (L = 6.02 × 10²³ mol⁻¹)
粒子数：N = n × L (L = 6.02 × 10²³ mol⁻¹)
2. Empirical and Molecular Formulae | 经验式与分子式
The empirical formula is the simplest whole‑number ratio of atoms in a compound. The molecular formula is a whole‑number multiple of the empirical formula.
经验式是化合物中原子的最简整数比。分子式是经验式的整数倍。
Multiplier n = Mᵣ(molecular) / Mᵣ(empirical)
倍数 n = 分子摩尔质量 / 经验式摩尔质量
Empirical formula from combustion data: convert masses of CO₂ and H₂O to moles of C and H, then find the simplest ratio.
由燃烧数据求经验式：将 CO₂ 和 H₂O 的质量换算为 C 和 H 的物质的量，进而求最简比。
3. Gas Calculations | 气体计算
The ideal gas law links pressure, volume, temperature and amount of gas. It is essential for both IB and Edexcel papers.
理想气体方程将压强、体积、温度与气体的物质的量联系起来，是IB与爱德思考试的核心公式。
pV = nRT (p in Pa, V in m³, T in K, R = 8.31 J K⁻¹ mol⁻¹)
pV = nRT (p 单位 Pa，V 单位 m³，T 单位 K，R = 8.31 J K⁻¹ mol⁻¹)
Boyle’s law: p₁V₁ = p₂V₂ at constant T
波义耳定律：恒温下 p₁V₁ = p₂V₂
Charles’s law: V₁ / T₁ = V₂ / T₂ at constant p
查理定律：恒压下 V₁ / T₁ = V₂ / T₂
Combined gas law: p₁V₁ / T₁ = p₂V₂ / T₂
联合气体定律：p₁V₁ / T₁ = p₂V₂ / T₂
Molar mass from gas density: M = mRT / (pV) or ρ = pM / (RT)
由气体密度求摩尔质量：M = mRT / (pV) 或 ρ = pM / (RT)
4. Thermochemistry and Enthalpy Changes | 热化学与焓变
Heat transferred in a reaction is often measured by temperature changes in a calorimeter.
反应中的热量转移常通过量热计中的温度变化来测定。
q = mcΔT (m = mass of solution, c = specific heat capacity, ΔT = temperature change)
q = mcΔT (m = 溶液质量，c = 比热容，ΔT = 温度变化)
ΔH = −q / n (mol of limiting reactant); ΔH = q / n for endothermic reactions treated as positive.
ΔH = −q / n (限制反应物的物质的量)；若定义吸热为正则 ΔH = q / n。
Hess’s law: ΔHreaction = ΣΔH°f(products) − ΣΔH°f(reactants)
盖斯定律：ΔH反应 = ΣΔH°f(生成物) − ΣΔH°f(反应物)
Using combustion enthalpies: ΔHreaction = ΣΔH°c(reactants) − ΣΔH°c(products)
利用燃烧焓：ΔH反应 = ΣΔH°c(反应物) − ΣΔH°c(生成物)
Bond enthalpy approximation: ΔH ≈ Σ(bond enthalpies broken) − Σ(bond enthalpies formed)
键焓近似：ΔH ≈ Σ(断裂键的键焓) − Σ(生成键的键焓)
5. Reaction Kinetics | 反应速率
The rate equation expresses how the rate depends on concentration of reactants. The order of reaction is determined experimentally.
速率方程表达了反应速率如何依赖于反应物浓度；反应级数由实验确定。
rate = k[A]ᵐ[B]ⁿ (m, n are orders; overall order = m + n)
rate = k[A]ᵐ[B]ⁿ (m、n 为级数；总级数 = m + n)
Units of k: mol dm⁻³ s⁻¹ divided by (mol dm⁻³)^(overall order).
k 的单位：mol dm⁻³ s⁻¹ 除以 (mol dm
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