📚 IB Chemistry Formula Handbook | IB 化学公式汇总手册
This IB Chemistry Formula Handbook consolidates essential equations and relationships required for the Diploma Programme. From mole calculations to electrochemistry, these formulas are the foundation for solving problems in both Standard Level and Higher Level. Understanding when and how to apply each formula is critical for success in examinations and internal assessments.
本 IB 化学公式手册汇总了文凭课程所需的关键方程和关系式。从摩尔计算到电化学，这些公式是解决标准水平和高水平问题的基础。理解何时以及如何应用每个公式对于考试和内部评估的成功至关重要。
1. The Mole and Stoichiometry | 摩尔与化学计量
The number of moles n is given by the mass of a substance divided by its molar mass.
物质的量 n 等于物质的质量除以摩尔质量。
n = m / M
Number of particles N relates to moles via Avogadro's constant L (6.02 × 10²³ mol⁻¹).
粒子数 N 通过阿伏伽德罗常数 L (6.02 × 10²³ mol⁻¹) 与摩尔数相关联。
N = n × L
Concentration c (mol·dm⁻³) is the amount of solute per unit volume of solution.
浓度 c (mol·dm⁻³) 是单位体积溶液中溶质的量。
c = n / V
When diluting a solution, the moles of solute remain constant.
稀释溶液时，溶质的摩尔数保持不变。
c₁V₁ = c₂V₂
or gases at standard conditions, the molar volume Vₘ = 22.7 dm³ mol⁻¹ (STP: 0°C, 100 kPa).
在标准状况下，气体的摩尔体积 Vₘ = 22.7 dm³ mol⁻¹ (STP：0°C，100 kPa)。
Vₘ = 22.7 dm³ mol⁻¹
2. Atomic Structure and Empirical Formula | 原子结构与经验式确定
Relative atomic mass Aᵣ is calculated from isotopic masses and their percentage abundances.
相对原子质量 Aᵣ 由同位素质量及其丰度百分比计算得出。
Aᵣ = Σ (isotopic mass × % abundance) / 100
The empirical formula gives the simplest whole‑number ratio of atoms; the molecular formula is a multiple of it.
经验式给出最简单的整数原子比；分子式是其整数倍。
Molecular formula = (Empirical formula)ₙ
The multiplier n equals the relative molecular mass divided by the empirical formula mass.
倍数 n 等于相对分子质量除以经验式质量。
n = Mᵣ / Mᵣ(empirical)
The relationships between speed of light c, wavelength λ, frequency ν and photon energy E are central to spectroscopy.
光速 c、波长 λ、频率 ν 和光子能量 E 之间的关系是光谱学的核心。
c = ν λ
E = h ν
3. The Ideal Gas Equation | 理想气体状态方程
The ideal gas law links pressure P (Pa), volume V (m³), amount n (mol) and temperature T (K).
理想气体定律将压强 P (Pa)、体积 V (m³)、物质的量 n (mol) 和温度 T (K) 联系起来。
PV = nRT
he The gas constant R = 8.31 J·K⁻¹·mol⁻¹. At STP, one mole of any ideal gas occupies 22.7 dm³.
气体常数 R = 8.31 J·K⁻¹·mol⁻¹。在 STP 下，1 mol 任何理想气体的体积为 22.7 dm³。
For a fixed mass of gas, the combined gas law can compare two sets of conditions.
对于一定质量的气体，可用联合气体定律比较两种状态。
P₁V₁ / T₁ = P₂V₂ / T₂
4. Energetics and Thermochemistry | 能量学与热化学
Heat absorbed or released by a substance is calculated from its mass, specific heat capacity and temperature change.
物质吸收或释放的热量由其质量、比热容和温度变化计算。
q = m c ΔT
Enthalpy change of a reaction (ΔH) is determined from the heat transferred and the amount of limiting reactant.
反应的焓变 (ΔH) 由传递的热量和限制反应物的量决定。
ΔH = –q / n
Hess's law allows the calculation of an overall ΔH from a series of intermediate steps.
赫斯定律允许通过一系列中间步骤计算总 ΔH。
ΔH°reaction = Σ ΔH°f(products) – Σ ΔH°f(reactants)
Enthalpy change can also be approximated using average bond enthalpies.
焓变也可以用平均键焓来近似估算。
ΔH ≈ Σ BE(bonds broken) – Σ BE(bonds formed)
5. Chemical Kinetics | 化学动力学
a reaction aA + bB → products, the rate law expresses how rate depends on concentrations.
对于反应 aA + bB → 产物，速率方程表达了速率如何依赖于浓度。
rate = k [A]ᵐ [B]ⁿ
The Arrhenius equation links the rate constant k to temperature and activation energy Eₐ.
阿伦尼乌斯方程将速率常数 k 与温度和活化能 Eₐ 联系起来。
ln k = ln A – Eₐ / (RT)
Alternatively, one can compare k values at two temperatures using the integrated form.
或者，可用积分形式比较两个温度下的 k 值。
ln(k₂ / k₁) = –(Eₐ / R)(1/T₂ – 1/T₁)
6. Chemical Equilibrium | 化学平衡
The equilibrium constant Kc is expressed in terms of concentrations raised to the stoichiometric coefficients.
平衡常数 Kc 以各组分的浓度（幂为化学计量数）表示。
Kc = [C]ᶜ [D]ᵈ / ([A]ᵃ [B]ᵇ)
For gaseous reactions, Kp uses partial pressures and relates to Kc via the change in moles of gas Δn.
对于气体反应，Kp 使用分压，并通过气体摩尔数的变化 Δn 与 Kc 关联。
Kp = Kc (RT)Δn
The standard Gibbs free energy change and K are related at a given temperature.
标准吉布斯自由能变与 K 在给定温度下相关联。
ΔG° = –RT ln K
The van 't Hoff equation describes how K varies with temperature.
范特霍夫方程描述了 K 随温度的变化。
ln(K₂ / K₁) = –(ΔH° / R)(1/T₂ – 1/T₁)
7. Acids and Bases | 酸碱
The pH of a solution is the negative logarithm of the hydrogen ion concentration.
溶液的 pH 是氢离子浓度的负对数。
pH = –log [H⁺]
Similarly, pOH = –log [OH⁻]. In water at 298 K, Kw = 1.0 × 10⁻¹⁴.
类似地，pOH = –log [OH⁻]。在 298 K 时，水的离子积 Kw = 1.0 × 10⁻¹⁴。
Kw = [H⁺][OH⁻] = 1.0 × 10⁻¹⁴
The acid dissociation constant Ka and its logarithmic form pKa indicate acid strength.
酸解离常数 Ka 及其对数形式 pKa 指示酸的强度。
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