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- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.10%3A_Heats_of_Fusion_and_SolidificationThis page explains the heat transfer process when holding an ice cube, highlighting how heat energy from the hand melts the ice without changing temperature due to the phase change. It covers the conc...This page explains the heat transfer process when holding an ice cube, highlighting how heat energy from the hand melts the ice without changing temperature due to the phase change. It covers the concepts of molar heat of fusion and solidification, noting that their values are equal but opposite. Additionally, it mentions calculations to determine heat absorbed or released, exemplified by the melting of 31.6 g of ice, which absorbs around 10.5 kJ.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/21%3A_Entropy_and_the_Third_Law_of_Thermodynamics/21.08%3A_Spectroscopic_Entropies_sometimes_disgree_with_Calorimetric_EntropiesThis page discusses the measurement of gas entropy, highlighting that inconsistencies known as residual entropy can emerge in certain substances. This occurs in materials with multiple configurations ...This page discusses the measurement of gas entropy, highlighting that inconsistencies known as residual entropy can emerge in certain substances. This occurs in materials with multiple configurations at absolute zero, challenging the third law of thermodynamics which asserts that entropy should be zero at that temperature. Examples like glass, ice, and carbon monoxide showcase residual entropy due to their imperfect crystal structures.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/15%3A_Water/15.08%3A_DissociationThis page discusses the hazards of winter ice on roads and sidewalks and the use of deicing salts like sodium chloride and calcium chloride to melt ice. It explains the dissociation of these ionic com...This page discusses the hazards of winter ice on roads and sidewalks and the use of deicing salts like sodium chloride and calcium chloride to melt ice. It explains the dissociation of these ionic compounds into individual ions when dissolved in water, contrasting this with nonionic compounds, such as sucrose, which do not dissociate. The importance of understanding these processes for effective winter road maintenance is also highlighted.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/19%3A_The_First_Law_of_Thermodynamics/19.10%3A_Relative_Enthalpies_Can_Be_Determined_from_Heat_Capacity_Data_and_Heats_of_TransitionThis page explains enthalpy, focusing on the significance of changes in enthalpy (ΔH) rather than absolute values. It covers three processes: heating ice, melting, and heating water, including related...This page explains enthalpy, focusing on the significance of changes in enthalpy (ΔH) rather than absolute values. It covers three processes: heating ice, melting, and heating water, including related ΔH calculations.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.12%3A_Multi-Step_Problems_with_Changes_of_StateThis page explains the energy-intensive process of converting ice at -30°C to steam at 140°C, which involves multiple steps: heating ice, melting it, heating water, vaporizing water, and heating steam...This page explains the energy-intensive process of converting ice at -30°C to steam at 140°C, which involves multiple steps: heating ice, melting it, heating water, vaporizing water, and heating steam. The total energy required for this transformation is calculated to be 133.4 kJ, with the highest energy absorption occurring during the vaporization phase.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/13%3A_States_of_Matter/13.20%3A_Phase_Diagram_for_WaterThis page explores the properties of snow and water, emphasizing that slightly wet snow is ideal for snowball making due to enhanced particle cohesion. It notes that ice is less dense than liquid wate...This page explores the properties of snow and water, emphasizing that slightly wet snow is ideal for snowball making due to enhanced particle cohesion. It notes that ice is less dense than liquid water, enabling it to float, and highlights a negative slope in the phase diagram between solid and liquid phases. Additionally, it defines the critical point at a temperature of 373.99°C and a pressure of 217.75 atm, indicating conditions where gas cannot be liquefied, regardless of pressure.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/15%3A_Water/15.02%3A_Structure_of_IceThis page explains that ice is less dense than liquid water because of hydrogen bonding and its hexagonal structure, allowing it to float. While ice has beneficial uses, such as cooling and recreation...This page explains that ice is less dense than liquid water because of hydrogen bonding and its hexagonal structure, allowing it to float. While ice has beneficial uses, such as cooling and recreation, it can also cause damage. As water cools, it reaches maximum density at 4°C before becoming less dense at freezing, which helps aquatic life survive under the ice during winter, preventing complete freezing of lakes.
