General Chemistry Final Cheat Sheet, Cheat Sheet of Chemistry

Download General Chemistry Final Cheat Sheet and more Cheat Sheet Chemistry in PDF only on Docsity! DAT General Chemistry Equation Sheet Chapter 0: General and Lab Concepts Review Dilutions 𝑀1𝑉1 = 𝑀2𝑉2 or 𝐶1𝑉1 = 𝐶2𝑉2 𝑀 𝑜𝑟 𝐶 = 𝑐𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛 𝑉 = 𝑣𝑜𝑙𝑢𝑚𝑒 Percent Error (𝐴 − 𝑇) 𝑇 × 100 𝑇 = 𝑡ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙 𝐴 = 𝑎𝑐𝑡𝑢𝑎𝑙 Absorbance (Spectro- photometer) 𝐴𝑏𝑠 = 𝜀𝑐𝑙 𝜀 = 𝑚𝑜𝑙𝑎𝑟 𝑒𝑥𝑡𝑖𝑛𝑐𝑡𝑖𝑜𝑛 𝑐𝑜𝑒𝑓𝑓𝑖𝑐𝑖𝑒𝑛𝑡 (𝑚𝑜𝑙𝑎𝑟 𝑎𝑏𝑠𝑜𝑟𝑝𝑡𝑖𝑣𝑖𝑡𝑦) 𝑐 = 𝑠𝑎𝑚𝑝𝑙𝑒′𝑠 𝑐𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛 𝑙 = 𝑝𝑎𝑡ℎ 𝑙𝑒𝑛𝑔𝑡ℎ Chapter 2: Atomic and Electronic Structure Energy of a photon 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 = ℎ𝑓 = ℎ𝑐 𝜆 ℎ = 𝑃𝑙𝑎𝑛𝑐𝑘 ′𝑠 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 (6.63 × 10−34𝐽 ∙ 𝑠) 𝑓 = 𝑝ℎ𝑜𝑡𝑜𝑛′𝑠 𝑓𝑟𝑒𝑞𝑢𝑒𝑛𝑐𝑦 𝑐 = 𝑠𝑝𝑒𝑒𝑑 𝑜𝑓 𝑙𝑖𝑔ℎ𝑡 (3.0 × 108 𝑚 𝑠⁄ ) 𝜆 = 𝑝ℎ𝑜𝑡𝑜𝑛′𝑠 𝑤𝑎𝑣𝑒𝑙𝑒𝑛𝑔𝑡ℎ Absorption/ Emission Line Spectra 𝛥𝐸 = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 Kinetic Energy of an electron (Photoelectric Effect) 𝐾𝐸𝑒− = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 − 𝜙 𝜙 = 𝑤𝑜𝑟𝑘 𝑓𝑢𝑛𝑐𝑡𝑖𝑜𝑛 (𝑚𝑖𝑛𝑖𝑚𝑢𝑚 𝑒𝑛𝑒𝑟𝑔𝑦 𝑛𝑒𝑒𝑑𝑒𝑑 𝑡𝑜 𝑖𝑜𝑛𝑖𝑧𝑒 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛) Chapter 7: Chemical Solutions Molarity 𝑀 = 𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒 𝐿𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 Molality 𝑚 = 𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒 𝑘𝑔𝑠𝑜𝑙𝑣𝑒𝑛𝑡 Henry’s Law 𝑃𝐴 = 𝑘𝐻[𝐴] 𝑃𝐴 = 𝑝𝑎𝑟𝑡𝑖𝑎𝑙 𝑝𝑟𝑒𝑠𝑠𝑢𝑟𝑒 𝑜𝑓 𝑔𝑎𝑠 𝐴 𝑘𝐻 = 𝐻𝑒𝑛𝑟𝑦 ′𝑠 𝐿𝑎𝑤 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 (𝑣𝑎𝑟𝑖𝑒𝑠 𝑝𝑒𝑟 𝑝𝑟𝑜𝑏𝑙𝑒𝑚) [A] = conc. of gas A Freezing Point Depression 𝛥𝑇𝐹 = −𝑖𝐾𝐹𝑚 𝑖 = 𝑣𝑎𝑛 ′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟 𝐾𝐹 = 𝐹. 𝑃. 𝑑𝑒𝑝𝑟𝑒𝑠𝑠𝑖𝑜𝑛 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑚 = 𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦 Boiling Point Elevation 𝛥𝑇𝐵 = 𝑖𝐾𝐵𝑚 𝑖 = 𝑣𝑎𝑛 ′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟 𝐾𝐵 = 𝐵. 𝑃. 𝑑𝑒𝑝𝑟𝑒𝑠𝑠𝑖𝑜𝑛 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑚 = 𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦 Vapor Pressure Depression (Raoult’s Law) 𝑃𝑠𝑜𝑙𝑛 = 𝜒𝑠𝑜𝑙𝑣𝑃𝑠𝑜𝑙𝑣 0 𝑃𝑠𝑜𝑙𝑛 = 𝑉𝑃 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝜒𝑠𝑜𝑙𝑣 = 𝑚𝑜𝑙 𝑓𝑟𝑎𝑐𝑡 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 𝑃𝑠𝑜𝑙𝑣 0 = 𝑉𝑃 𝑜𝑓 𝑝𝑢𝑟𝑒 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 Osmotic Pressure (𝝅) 𝜋 = 𝑖𝑀𝑅𝑇 𝑀 = 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑖 = 𝑣𝑎𝑛′𝑡 𝐻𝑜𝑓𝑓 𝑓𝑎𝑐𝑡𝑜𝑟 𝑅 = 0.0821 𝐿 ⋅ 𝑎𝑡𝑚 𝑚𝑜𝑙 ⋅ 𝐾 𝑇 = 𝑡𝑒𝑚𝑝. 𝑖𝑛 𝐾𝑒𝑙𝑣𝑖𝑛 Chapter 5: Gases Pressure 𝑃 = 𝐹 𝐴 𝐹 = 𝑓𝑜𝑟𝑐𝑒 𝐴 = 𝑎𝑟𝑒𝑎 Average Kinetic Energy 𝐾𝐸𝑎𝑣𝑔 = 3 2⁄ 𝑅𝑇 𝑅 = 8.314 𝐽 𝑚𝑜𝑙 ∙ 𝐾 Root-Mean- Square Speed (𝒗) 𝑣 = √ 3𝑅𝑇 𝑀𝑚 𝑅 = 8.314 𝐽 𝑚𝑜𝑙 ∙ 𝐾 𝑀𝑚 = 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 Ideal Gas Law 𝑃𝑉 = 𝑛𝑅𝑇 𝑛 = # 𝑜𝑓 𝑚𝑜𝑙𝑒𝑠 𝑅 = 0.0821 𝐿 ⋅ 𝑎𝑡𝑚 𝑚𝑜𝑙 ⋅ 𝐾 Boyle’s Law 𝑉 ∝ 1 𝑃 Charles’ Law 𝑉 ∝ 𝑇 Avogadro’s Law 𝑉 ∝ 𝑛 Combined Gas Law 𝑃1𝑉1 𝑛1𝑇1 = 𝑃2𝑉2 𝑛2𝑇2 Standard Temp. & Pressure (STP) P=1 atm T=273 K *1 mol of gas = 22.4 L at STP Standard Conditions All aqueous species @ 1M All gaseous species @1 atm T=298 K Density 𝑃(𝑀𝑀) 𝑅𝑇 = 𝑚 𝑣 𝑀𝑀 = 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑅 = 0.0821 𝐿 ⋅ 𝑎𝑡𝑚 𝑚𝑜𝑙 ⋅ 𝐾 𝑚 = 𝑚𝑎𝑠𝑠 𝑣 = 𝑣𝑜𝑙𝑢𝑚𝑒 Dalton’s Law of Partial Pressures 𝑃𝑡𝑜𝑡𝑎𝑙 = 𝑃𝐴 + 𝑃𝐵 + ⋯ Dalton’s Law of Partial Pressures 𝑃𝐴 = 𝜒𝐴𝑃𝑡𝑜𝑡𝑎𝑙 𝜒𝐴 = 𝑚𝑜𝑙 𝑓𝑟𝑎𝑐𝑡𝑖𝑜𝑛 𝑜𝑓 𝑔𝑎𝑠 𝐴 Graham’s Law of Effusion 𝑟1 𝑟2 = √ 𝑀𝑚2 𝑀𝑚1 𝑟 = 𝑟𝑎𝑡𝑒 𝑜𝑓 𝑒𝑓𝑓𝑢𝑠𝑖𝑜𝑛 𝑀 = 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 Real Gas Equation (𝑃 + 𝑎𝑛2 𝑉2 )(𝑉 − 𝑛𝑏) = 𝑛𝑅𝑇 𝑎 & 𝑏 = 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡𝑠 𝑠𝑝𝑒𝑐𝑖𝑓𝑖𝑐 𝑡𝑜 𝑒𝑎𝑐ℎ 𝑔𝑎𝑠 𝑎𝑛2 𝑉2 𝑐𝑜𝑟𝑟𝑒𝑐𝑡𝑠 𝑓𝑜𝑟 𝐼𝑀𝐹𝑠 −𝑛𝑏 𝑐𝑜𝑟𝑟𝑒𝑐𝑡𝑠 𝑓𝑜𝑟 𝑣𝑜𝑙𝑢𝑚𝑒 Chapter 8: Chemical Kinetics General Rate Law A + B → C + D 𝑟𝑎𝑡𝑒 = 𝑘[𝐴]𝑚[𝐵]𝑛 𝑘 = 𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑚 & 𝑛 = 𝑑𝑒𝑡𝑒𝑟𝑚𝑖𝑛𝑒𝑑 e𝑥𝑝𝑒𝑟𝑖𝑚𝑒𝑛𝑡𝑎𝑙𝑙𝑦 Rate Constant Units 0 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀1 ∙ 𝑠−1 1𝑠𝑡 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑠−1 2𝑛𝑑 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀−1 ∙ 𝑠−1 3𝑟𝑑 𝑜𝑟𝑑𝑒𝑟: 𝑘 = 𝑀−2 ∙ 𝑠−1 𝑘 = 𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑀 = 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦 s= 𝑠𝑒𝑐𝑜𝑛𝑑𝑠 Arrhenius Equation 𝑘 = 𝐴𝑒−𝐸𝑎 𝑅𝑇⁄ 𝑘 = 𝑟𝑎𝑡𝑒 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝐴 = 𝑢𝑛𝑖𝑞𝑢𝑒 𝑡𝑜 𝑒𝑎𝑐ℎ 𝑟𝑥𝑛 𝐸𝑎 = 𝑎𝑐𝑡. 𝑒𝑛𝑒𝑟𝑔𝑦 𝑅 = 8.314 𝐽 𝑚𝑜𝑙 ∙ 𝐾 𝑇 = 𝑡𝑒𝑚𝑝. 𝑖𝑛 𝐾𝑒𝑙𝑣𝑖𝑛