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- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.16%3A_Standard_Heat_of_FormationThis page discusses the Hope diamond, valued at $350 million, and compares it to graphite, which is much cheaper. It explains that the differences between these two forms of carbon arise from their di...This page discusses the Hope diamond, valued at $350 million, and compares it to graphite, which is much cheaper. It explains that the differences between these two forms of carbon arise from their distinct organizational structures and formation conditions. It also defines standard heat of formation (ΔHof), describing it as the enthalpy change involved in forming a mole of a compound from its elements at specified standard conditions.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/23%3A_Electrochemistry/23.11%3A_ElectroplatingThis page discusses the astrolabe, a brass instrument used for studying planetary motions and astrology, and electroplating, a decorative method that deposits metals onto surfaces via an electrolytic ...This page discusses the astrolabe, a brass instrument used for studying planetary motions and astrology, and electroplating, a decorative method that deposits metals onto surfaces via an electrolytic cell. The process uses copper sulfate and a copper anode to ensure consistent copper ion concentration, with the possibility of using other metals like chromium, gold, silver, and platinum in the technique.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/23%3A_Electrochemistry/23.01%3A_Direct_Redox_ReactionsThis page discusses the popularity of gold and silver in jewelry owing to their stability. It explains a redox reaction where zinc displaces copper from copper(II) sulfate, showcasing zinc's higher re...This page discusses the popularity of gold and silver in jewelry owing to their stability. It explains a redox reaction where zinc displaces copper from copper(II) sulfate, showcasing zinc's higher reactivity. The text highlights spontaneous versus nonspontaneous reactions, noting that copper cannot oxidize zinc, leading to no reaction when copper is introduced to zinc ions.
