Title | Main dat-general-chemistry-equation-sheet |
---|---|
Author | Esra Fidancı |
Course | Practical Chemistry I |
Institution | University of Birmingham |
Pages | 2 |
File Size | 196.4 KB |
File Type | |
Total Downloads | 16 |
Total Views | 148 |
chemistry formula sheet...
DAT General Chemistry Equation Sheet Gases/Gas Laws
General Concepts
Density: (d = m/v) Dilutions: M1V1 = M2V2 (or C1V1 = C2V2) % Error Calculations % 𝐸𝑟𝑟𝑜𝑟 =
𝐴𝑐𝑡𝑢𝑎𝑙 − 𝑡ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙 𝑥100 𝑡ℎ𝑒𝑜𝑟𝑒𝑡𝑖𝑐𝑎𝑙
Spectrophotometer: 𝐴𝑏𝑠 =
ɛ𝑐𝑙
Root-mean-square speed: 𝑣 = √ 𝑀
Absorption/Emission Line Spectra: 𝛥𝐸 = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 ℎ𝑐 Energy of a photon: 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 = ℎ𝑓 = 𝜆 ∗ 108 𝑚⁄
𝑐 = 3.0 𝑠 ℎ = 6.63 ∗ 10−34 𝐽 · 𝑠
Photoelectric Effect: 𝐾𝐸𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛 = 𝐸𝑝ℎ𝑜𝑡𝑜𝑛 − 𝜙
𝜙 = 𝑤𝑜𝑟𝑘 𝑓𝑢𝑛𝑐𝑡𝑖𝑜𝑛 (𝑚𝑖𝑛𝑖𝑚𝑢𝑚 𝑒𝑛𝑒𝑟𝑔𝑦 𝑡𝑜 𝑖𝑜𝑛𝑖𝑧𝑒 𝑒𝑙𝑒𝑐𝑡𝑟𝑜𝑛)
Chemical Kinetics and Equilibrium
General Rate Law: 𝑟𝑎𝑡𝑒 = 𝑘[𝐴]𝑚 [𝐵]𝑛
Arrhenius Equation: 𝑘 = 𝐴𝑒 −𝐸𝑎⁄𝑅𝑇 Equilibrium Constant:
𝐾𝑃 =
𝑃𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠
𝑃𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠
𝑬𝒂 = activation energy R = 0.0821 L atm/mol K
Solutions
Boyle’s Law:
𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 (𝑀) = 𝐿𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑚𝑜𝑙𝑒𝑠𝑠𝑜𝑙𝑢𝑡𝑒 𝑚𝑜𝑙𝑎𝑙𝑖𝑡𝑦 (𝑚) = 𝑘𝑔𝑠𝑜𝑙𝑣𝑒𝑛𝑡
Henry’s Law: 𝑃𝐴 = 𝑘𝐻 [𝐴]
Colligative Properties Freezing Point Depression: Boiling Point Elevation: Raoult’s Law (* = pure): Osmotic Pressure:
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𝑲𝑭 /𝑲𝑩 = F.P/B.P depression/elevation constant 𝝌𝑨 = mole fraction of A i = van’t Hoff Factor R = 0.0821 L atm/mol K M = molarity, m = molality
𝛥𝑇𝐹 = −𝑖𝐾𝐹 𝑚 𝛥𝑇𝐵 = 𝑖𝐾𝐵 𝑚 𝑃𝐴 = 𝜒𝐴 𝑃𝐴 ∗ 𝜋 = 𝑖𝑀𝑅𝑇
𝑚
𝑃∝
1 𝑉
𝑃1 𝑉1
=
𝑉∝ 𝑇 𝑉∝ n
𝑛1 𝑇1
Combined Gas Law:
𝑃2 𝑉2
𝑛2 𝑇2
Dalton’s Law of Partial Pressures: 𝑃𝑇𝑜𝑡 = 𝑃𝐴 + 𝑃𝐵 + ⋯ 𝑃𝐴 = 𝜒𝐴 ∗ 𝑃𝑇𝑜𝑡 𝜒𝐴 = 𝑚𝑜𝑙 𝑓𝑟𝑎𝑐𝑡𝑖𝑜𝑛 𝐴
Grahams Law of Effusion: 𝑟1 𝑀𝑚2 =√ 𝑟2 𝑀𝑚1
R = 0.0821 L atm/mol K n = moles 𝑴𝒎 = molar mass r = rate of effusion a and b are constants specific to a given gas
Acid-Base pH Scale 𝑝𝐻 = −log[𝐻 +]
[𝐻 +] = 10−𝑝𝐻
𝑝𝐻 + 𝑝𝑂𝐻 = 14
[𝐻 +][𝑂𝐻−] = 1 ∗ 10−14
𝑝𝑂𝐻 = −log [𝑂𝐻−]
Weak Acids:
Concentration
3𝑅𝑇
𝑃𝑉 = 𝑛𝑅𝑇
Ideal Gas Law: Charles’ Law: Avogadro’s Law:
Atomic Structure
𝐾𝑐 =
𝐾. 𝐸. 𝑎𝑣𝑔 = 3⁄2 𝑅𝑇 (𝑝𝑒𝑟 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑔𝑎𝑠)
Gas Laws
Abs = Absorbance ɛ = molar extinction coefficient (molar absorptivity) l = path length
[𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠] [𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠]
Pressure: 𝑃 = 𝐹𝑜𝑟𝑐𝑒/𝐴𝑟𝑒𝑎 Average Kinetic Energy:
𝐾𝑎 =
[𝑂𝐻−] = 10−𝑝𝐻
[𝐻3 𝑂+ ][𝐴− ]
[𝐻 +] = √𝐾𝑎 [𝐻𝐴]
[𝐻𝐴]
Weak Bases:
𝐾𝑏 =
[𝑂𝐻 − ][𝐻𝐴] [𝐴− ]
[𝑂𝐻−] = √𝐾𝑏 [𝐵]
𝐾𝑎 ∗ 𝐾𝑏 = 𝐾𝑤
Buffer: 𝑝𝐻 = 𝑝𝐾𝑎 + log
[𝐴− ] [𝐻𝐴]
Titration/Neutralization: 𝑛𝐴 𝑀𝐴 𝑉𝐴 = 𝑛𝐵 𝑀𝐵 𝑉𝐵
DAT General Chemistry Equation Sheet Thermodynamics/Thermochemistry
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
Electrochemical Cells Standard Cell Potentials ɛ° = ɛ° 𝑟𝑒𝑑 + ɛ°𝑜𝑥 ɛ° = ɛ°𝑐𝑎𝑡ℎ𝑜𝑑𝑒 + ɛ° 𝑎𝑛𝑜𝑑𝑒 Nernst Equation (non-standard cell potentials)
𝐸 = 𝐸° −
0.0592 𝑛
log 𝑄
Faraday’s Law (quantitative calculations) 𝐼 ∗ 𝑡𝑠 ∗ 𝑀𝑊𝑝𝑟𝑜𝑑𝑢𝑐𝑡 = 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑛∗𝐹 𝐼 ∗ 𝑡𝑠 = 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑛∗𝐹
I = current, 𝒕𝒔 = time in seconds, n = moles, F = Faraday’s constant (96485 𝑐𝑜𝑢𝑙𝑜𝑚𝑏𝑠⁄𝑚𝑜𝑙 ), Q = reaction quotient
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
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Nuclear Reactions
Kinetics (always 1st order) 𝑁 = 𝑁0 𝑒 −𝑘𝑡 ln 𝑁 = ln 𝑁0 − 𝑘𝑡 Nuclear Binding Energy: 𝐸 = 𝛥𝑚𝑐 2 (𝛥𝑚 must be in kg)
k = reaction constant
m = mass c = speed of light...