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- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/15%3A_Water/15.06%3A_Liquid-Liquid_SolutionsThis page discusses the 2010 Gulf of Mexico oil spill, highlighting how the nonpolar nature of crude oil prevents it from mixing with water. It explains the concept of miscibility, noting that nonpola...This page discusses the 2010 Gulf of Mexico oil spill, highlighting how the nonpolar nature of crude oil prevents it from mixing with water. It explains the concept of miscibility, noting that nonpolar compounds like oil do not dissolve in polar solvents, emphasizing the principle "like dissolves like" and the necessity of polarity for solubility in water through hydrogen bonding.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/16%3A_Solutions/16.07%3A_Percent_SolutionsThis page discusses the variation in numerical recognition across cultures, noting that some do not count beyond three. It highlights American cultural practices in expressing solution concentrations,...This page discusses the variation in numerical recognition across cultures, noting that some do not count beyond three. It highlights American cultural practices in expressing solution concentrations, defining concentrated and dilute solutions, and explaining how concentrations can be represented in mass percent and volume percent. The page includes examples to illustrate methods for calculating these percentages.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/04%3A_Putting_the_First_Law_to_Work/4.06%3A_Useful_Definitions_and_RelationshipsThis chapter outlines several important thermodynamic definitions and relationships, such as heat capacities, coefficient of thermal expansion, and isothermal compressibility. It demonstrates how thes...This chapter outlines several important thermodynamic definitions and relationships, such as heat capacities, coefficient of thermal expansion, and isothermal compressibility. It demonstrates how these can be used to derive useful expressions and solve problems, like determining changes in enthalpy during isothermal compression.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/25%3A_Organic_Chemistry/25.13%3A_EstersThis page discusses the composition and extraction of perfumes, highlighting that they are mainly sourced from around 2,000 plant species. Methods like solvent extraction and distillation are used, an...This page discusses the composition and extraction of perfumes, highlighting that they are mainly sourced from around 2,000 plant species. Methods like solvent extraction and distillation are used, and oil dilution in ethanol impacts pricing. Key components are esters, which are organic compounds influential in creating scents, with unique properties related to boiling points and solubility. Esters play a significant role in the natural odors and flavors of plants.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/14%3A_The_Behavior_of_Gases/14.10%3A_Gas_StoichiometryThis page discusses the Haber cycle's importance in ammonia production, emphasizing the need for excess nitrogen and hydrogen. It highlights the use of stoichiometry, molar volume, and the ideal gas l...This page discusses the Haber cycle's importance in ammonia production, emphasizing the need for excess nitrogen and hydrogen. It highlights the use of stoichiometry, molar volume, and the ideal gas law for calculating gas reactions under various conditions. An example showcases the combustion of ethanol, demonstrating how 25.21 g produces 1.094 moles of CO2, with the ideal gas law determining the produced volume of 30.6 L.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.14%3A_Heat_of_CombustionThis page discusses the use of ethanol in gasoline to enhance fuel efficiency due to its high octane rating, despite potential increases in air pollution. It explains the concept of molar heat of comb...This page discusses the use of ethanol in gasoline to enhance fuel efficiency due to its high octane rating, despite potential increases in air pollution. It explains the concept of molar heat of combustion, which measures the energy released during combustion reactions involving carbon and oxygen, producing carbon dioxide and water. The molar heat of combustion for ethanol is noted as 1370 kJ/mol, and bomb calorimetry is mentioned as a method for this measurement.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/13%3A_States_of_Matter/13.08%3A_Vapor_PressureThis page explains the drinking duck toy as a demonstration of vapor pressure principles. It describes how sealing the container leads to evaporation and vapor pressure exertion, establishing dynamic ...This page explains the drinking duck toy as a demonstration of vapor pressure principles. It describes how sealing the container leads to evaporation and vapor pressure exertion, establishing dynamic equilibrium between liquid and vapor phases. The summary highlights the relationship between vapor pressure and temperature, noting that stronger intermolecular forces lead to lower vapor pressures and weaker forces result in higher pressures.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/16%3A_An_Introduction_to_Infrared_Spectrometry/16.01%3A_Theory_of_Infrared_Absorption_SpectrometryTo absorb an infrared photon, the absorbing species must experience a change in its dipole moment, which allows the oscillation in the photon's electrical field to interact with an oscillation in char...To absorb an infrared photon, the absorbing species must experience a change in its dipole moment, which allows the oscillation in the photon's electrical field to interact with an oscillation in charge within the absorbing species. If the two oscillations have the same frequency, then absorption is possible. In this section we consider classical and quantum mechanical models for vibrational spectrscopy.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/14%3A_The_Behavior_of_Gases/14.11%3A_Real_and_Ideal_GasesThis page discusses how molecular structure affects behavior, exemplified by ethanol and dimethylether's differing boiling points due to intermolecular interactions. It also covers the ideal gas law, ...This page discusses how molecular structure affects behavior, exemplified by ethanol and dimethylether's differing boiling points due to intermolecular interactions. It also covers the ideal gas law, noting that real gases deviate from ideal behavior at high pressures and low temperatures, with lighter gases like helium being more ideal than those with stronger intermolecular forces.
