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DAT General Chemistry Equation Sheet
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Thermodynamics/Thermochemistry
Electrochemical Cells
Nuclear Reactions
1st Law of Thermodynamics: ๐ฅ๐ธ = ๐ + ๐ค Work: ๐ค = โ๐๐ฅ๐ Calorimetry: ๐ = ๐ถ๐ฅ๐ ๐ = ๐๐๐ฅ๐ ๐ถ = โ๐๐๐ก ๐๐๐๐๐๐๐ก๐ฆ ๐ = ๐ ๐๐๐๐๐๐๐ โ๐๐๐ก q = heat added or removed from system m = mass Entropy ๐ฅ๐ = ๐ด๐๐๐๐๐๐๐ข๐๐ก๐ โ ๐ด๐๐๐๐๐๐๐ก๐๐๐ก๐ ๐๐๐๐ > ๐๐๐๐๐ข๐๐ > ๐๐ ๐๐๐๐ ๐๐๐ > ๐๐ ๐๐๐๐
Enthalpy (๐ฅ๐ป > 0) โ Endothermic (๐ฅ๐ป < 0) โ Exothermic
Enthalpies of Formation: ๐ฅ๐ป = ๐ด๐๐ฅ๐ปยฐ๐,๐๐๐๐๐ข๐๐ก๐ โ ๐ด๐๐ฅ๐ปยฐ๐,๐๐๐๐๐ก๐๐๐ก๐
Bond Dissociation Energy ๐ฅ๐ป = ๐ด๐ท๐๐๐๐๐ก๐๐๐ก๐ โ ๐ด๐ท๐๐๐๐๐ข๐๐ก๐ = ๐ด๐ท๐๐๐๐๐๐ โ ๐ด๐ท๐๐๐๐๐๐
Gibbs Free Energy ๐ฅ๐บ = ๐ฅ๐บยฐ + ๐ ๐๐๐๐ (nonstandard conditions, Q = reaction
quotient) ๐ฅ๐บยฐ = โ๐ ๐๐๐๐พ๐๐ ๐ฅ๐บยฐ = ๐ฅ๐ปยฐ โ ๐๐ฅ๐ยฐ 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 ษยฐ = ษยฐ๐๐๐ + ษยฐ๐๐ฅ ษยฐ = ษยฐ๐๐๐กโ๐๐๐ + ษยฐ๐๐๐๐๐ Nernst Equation (non-standard cell potentials) ๐ธ = ๐ธยฐ โ 0.0592
๐log ๐
Faradayโs Law (quantitative calculations) ๐ผ โ ๐ก๐ โ ๐๐๐๐๐๐๐ข๐๐ก
๐ โ ๐น= ๐๐๐ ๐ ๐๐ ๐๐๐๐๐ข๐๐ก
๐ผ โ ๐ก๐
๐ โ ๐น= ๐๐๐๐๐ ๐๐ ๐๐๐๐๐ข๐๐ก
I = current, ๐๐ = time in seconds, n = moles, F = Faradayโs constant (96485 ๐๐๐ข๐๐๐๐๐
๐๐๐โ ), Q = reaction quotient
Kinetics (always 1st order) ๐ = ๐0๐โ๐๐ก ln ๐ = ln ๐0 โ ๐๐ก Nuclear Binding Energy: ๐ธ = ๐ฅ๐๐2 (๐ฅ๐ must be in kg)
k = reaction constant
m = mass c = speed of light