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- https://chem.libretexts.org/Courses/Western_Washington_University/Biophysical_Chemistry_(Smirnov_and_McCarty)/01%3A_Biochemical_Thermodynamics/1.03%3A_ThermochemistryIn this chapter we apply the first law of thermodynamics and the concept of enthalpy introduced in Chapter I.2 to chemical reactions. At standard state conditions we can use tabulated heats of formati...In this chapter we apply the first law of thermodynamics and the concept of enthalpy introduced in Chapter I.2 to chemical reactions. At standard state conditions we can use tabulated heats of formation to calculate the change in enthalpy for any reaction. At temperatures other than standard conditions we use the temperature dependence of the enthalpy to derive an expression for the change in enthalpy of a reaction at any temperature in relation to a reference temperature.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/15%3A_Thermodynamics-_Atoms_Molecules_and_Energy/15.11%3A_Bond_Enthalpies_and_Exothermic_or_Endothermic_ReactionsThe bond enthalpy of the O―H bond is not much different in magnitude from those of the C―H and O=O bonds which it replaces: All lie between 400 and 500 kJ mol –1 . The determining factor making this r...The bond enthalpy of the O―H bond is not much different in magnitude from those of the C―H and O=O bonds which it replaces: All lie between 400 and 500 kJ mol –1 . The determining factor making this reaction exothermic is the exceedingly large bond enthalpy of the C=O bond which at 803 kJ mol –1 is almost twice as great as for the other bonds involved in the reaction.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Concept_Development_Studies_in_Chemistry_(Hutchinson)/10%3A_Energetics_of_Chemical_ReactionsThe heat released or consumed in a chemical reaction is typically amongst the most easily observed and most readily appreciated consequences of the reaction. Many chemical reactions are performed rout...The heat released or consumed in a chemical reaction is typically amongst the most easily observed and most readily appreciated consequences of the reaction. Many chemical reactions are performed routinely specifically for the purpose of utilizing the heat released by the reaction.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/03%3A_First_Law_of_Thermodynamics/3.04%3A_CalorimetryThis page discusses the importance of understanding thermodynamics in chemical reactions, particularly focusing on calorimetry to measure the heat exchange (\(q\)) during chemical reactions. It outlin...This page discusses the importance of understanding thermodynamics in chemical reactions, particularly focusing on calorimetry to measure the heat exchange (\(q\)) during chemical reactions. It outlines the use of bomb calorimetry, which is typically employed for combustion reactions. The process involves calculating the change in internal energy using a bomb calorimeter and examples to determine the enthalpy of combustion for substances.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Chemical_Reactions/Stoichiometry/Reaction_EquationsThe most important aspect of a chemical reaction is to know what are the reactants and what are the products. For this, the best description of a reaction is to write an equation for the reaction. A c...The most important aspect of a chemical reaction is to know what are the reactants and what are the products. For this, the best description of a reaction is to write an equation for the reaction. A chemical reaction equation gives the reactants and products, and a balanced chemical reaction equation shows the mole relationships of reactants and products. Often, the amount of energy involved in the reaction is given.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Basic_Principles_of_Organic_Chemistry_(Roberts_and_Caserio)/04%3A_Alkanes/4.04%3A_Combustion._Heats_of_Reaction._Bond_EnergiesAll hydrocarbons are attacked by oxygen at elevated temperatures and, if oxygen is in excess, complete combustion occurs to carbon dioxide and water. The heat evolved in this process - the heat of the...All hydrocarbons are attacked by oxygen at elevated temperatures and, if oxygen is in excess, complete combustion occurs to carbon dioxide and water. The heat evolved in this process - the heat of the combustion reaction, is a measure of the amount of energy stored in the C-C and C-H bonds of the hydrocarbon COMPARED to the energy stored in the products, carbon dioxide and water.
- https://chem.libretexts.org/Sandboxes/khaas/Inorganic_Chemistry_II_(CHEM4210)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.06%3A_Metallurgy/4.1.6.03%3A_The_Extraction_of_IronThis page looks at the use of the Blast Furnace in the extraction of iron from iron ore, and the conversion of the raw iron from the furnace into various kinds of steel. Contributors and Attributions ...This page looks at the use of the Blast Furnace in the extraction of iron from iron ore, and the conversion of the raw iron from the furnace into various kinds of steel. Contributors and Attributions Jim Clark (Chemguide.co.uk) Prof. Robert J. Lancashire (The Department of Chemistry, University of the West Indies)
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.08%3A_Thermochemical_EquationsThis page discusses the rising costs of home heating and the importance of choosing the right fuel based on thermochemical data. It highlights the exothermic nature of methane combustion, releasing 89...This page discusses the rising costs of home heating and the importance of choosing the right fuel based on thermochemical data. It highlights the exothermic nature of methane combustion, releasing 890.4 kJ, compared to the endothermic decomposition of calcium carbonate, which absorbs 177.8 kJ. Understanding thermochemical equations and the heat of reaction is vital for energy transfer and efficiency in heating systems.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/09%3A_Chemical_Equilibria/9.07%3A_The_Dumas_Bulb_Method_for_Measuring_Decomposition_EquilibriumThe Dumas Bulb experiment is a method to study the temperature-dependent dissociation of N2O4 gas, commonly used in physical chemistry labs. The experiment measures the dissociation degree by equilibr...The Dumas Bulb experiment is a method to study the temperature-dependent dissociation of N2O4 gas, commonly used in physical chemistry labs. The experiment measures the dissociation degree by equilibrium gas density at varying temperatures in a calibrated glass bulb. A formula calculates dissociation, factoring in measured versus theoretical densities, and an equilibrium constant is derived. The data enables the construction of a van't Hoff plot, providing insights into reaction enthalpy.
- https://chem.libretexts.org/Courses/Winona_State_University/Klein_and_Straumanis_Guided/04%3A_Alkanes_and_Cycloalkanes/4.21%3A_4-5_Combustion._Heats_of_Reaction._Bond_EnergiesAll hydrocarbons are attacked by oxygen at elevated temperatures and, if oxygen is in excess, complete combustion occurs to carbon dioxide and water. The heat evolved in this process - the heat of the...All hydrocarbons are attacked by oxygen at elevated temperatures and, if oxygen is in excess, complete combustion occurs to carbon dioxide and water. The heat evolved in this process - the heat of the combustion reaction, is a measure of the amount of energy stored in the C-C and C-H bonds of the hydrocarbon COMPARED to the energy stored in the products, carbon dioxide and water.
- https://chem.libretexts.org/Courses/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.06%3A_Metallurgy/4.1.6.03%3A_The_Extraction_of_IronThis page looks at the use of the Blast Furnace in the extraction of iron from iron ore, and the conversion of the raw iron from the furnace into various kinds of steel. Contributors and Attributions ...This page looks at the use of the Blast Furnace in the extraction of iron from iron ore, and the conversion of the raw iron from the furnace into various kinds of steel. Contributors and Attributions Jim Clark (Chemguide.co.uk) Prof. Robert J. Lancashire (The Department of Chemistry, University of the West Indies)
