DAT General Chemistry Equation Sheet

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Thermodynamics/Thermochemistry

Electrochemical Cells

Nuclear Reactions

1st Law of Thermodynamics: 𝛥𝐸 = 𝑞 + 𝑤 Work: 𝑤 = −𝑃𝛥𝑉 Calorimetry: 𝑞 = 𝐶𝛥𝑇 𝑞 = 𝑚𝑐𝛥𝑇 𝐶 = ℎ𝑒𝑎𝑡 𝑐𝑎𝑝𝑎𝑐𝑖𝑡𝑦 𝑐 = 𝑠𝑝𝑒𝑐𝑖𝑓𝑖𝑐 ℎ𝑒𝑎𝑡 q = heat added or removed from system m = mass Entropy 𝛥𝑆 = 𝛴𝑛𝑆𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠 − 𝛴𝑛𝑆𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 𝑆𝑔𝑎𝑠 > 𝑆𝑙𝑖𝑞𝑢𝑖𝑑 > 𝑆𝑠𝑜𝑙𝑖𝑑 𝑆𝑎𝑞 > 𝑆𝑠𝑜𝑙𝑖𝑑

Enthalpy (𝛥𝐻 > 0) – Endothermic (𝛥𝐻 < 0) – Exothermic

Enthalpies of Formation: 𝛥𝐻 = 𝛴𝑛𝛥𝐻°𝑓,𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠 − 𝛴𝑛𝛥𝐻°𝑓,𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠

Bond Dissociation Energy 𝛥𝐻 = 𝛴𝐷𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 − 𝛴𝐷𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠 = 𝛴𝐷𝑏𝑟𝑜𝑘𝑒𝑛 − 𝛴𝐷𝑓𝑜𝑟𝑚𝑒𝑑

Gibbs Free Energy 𝛥𝐺 = 𝛥𝐺° + 𝑅𝑇𝑙𝑛𝑄 (nonstandard conditions, Q = reaction

quotient) 𝛥𝐺° = −𝑅𝑇𝑙𝑛𝐾𝑒𝑞 𝛥𝐺° = 𝛥𝐻° − 𝑇𝛥𝑆° Standard Conditions All aqueous species @ 1M, all gaseous species @1 atm, T=298k Standard Temperature and Pressure T = 273K, P = 1 atm

Standard Cell Potentials ɛ° = ɛ°𝑟𝑒𝑑 + ɛ°𝑜𝑥 ɛ° = ɛ°𝑐𝑎𝑡ℎ𝑜𝑑𝑒 + ɛ°𝑎𝑛𝑜𝑑𝑒 Nernst Equation (non-standard cell potentials) 𝐸 = 𝐸° − 0.0592

𝑛log 𝑄

Faraday’s Law (quantitative calculations) 𝐼 ∗ 𝑡𝑠 ∗ 𝑀𝑊𝑝𝑟𝑜𝑑𝑢𝑐𝑡

𝑛 ∗ 𝐹= 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡

𝐼 ∗ 𝑡𝑠

𝑛 ∗ 𝐹= 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡

I = current, 𝒕𝒔 = time in seconds, n = moles, F = Faraday’s constant (96485 𝑐𝑜𝑢𝑙𝑜𝑚𝑏𝑠

𝑚𝑜𝑙⁄ ), Q = reaction quotient

Kinetics (always 1st order) 𝑁 = 𝑁0𝑒−𝑘𝑡 ln 𝑁 = ln 𝑁0 − 𝑘𝑡 Nuclear Binding Energy: 𝐸 = 𝛥𝑚𝑐2 (𝛥𝑚 must be in kg)

k = reaction constant

m = mass c = speed of light