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- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.04%3A_Heat_Capacity_and_Specific_HeatThis page explains heat capacity and specific heat, emphasizing their effects on temperature changes in objects. It illustrates how mass and chemical composition influence heating rates, using a wadin...This page explains heat capacity and specific heat, emphasizing their effects on temperature changes in objects. It illustrates how mass and chemical composition influence heating rates, using a wading pool versus a larger swimming pool as an example. Water's high specific heat (4.18 J/g°C) requires more energy to warm up compared to other substances like metals, making it an effective coolant and contributing to moderate coastal climates.
- 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/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/17%3A_Thermochemistry/17.07%3A_CalorimetryThis page explains calorimetry, which measures heat transfer in chemical reactions and physical processes using a calorimeter. Originally, food calories were measured with a bomb calorimeter, but are ...This page explains calorimetry, which measures heat transfer in chemical reactions and physical processes using a calorimeter. Originally, food calories were measured with a bomb calorimeter, but are now determined based on protein, carbohydrate, and fat content. Temperature changes in the surrounding liquid reveal if a reaction is exothermic or endothermic, allowing for the calculation of heat transfer using the liquid's mass, specific heat, and temperature change.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/20%3A_Entropy_and_The_Second_Law_of_Thermodynamics/20.03%3A_Unlike_heat_Entropy_is_a_State_FunctionThis page discusses entropy as a state function that integrates to zero over circular paths returning to initial conditions. It examines a path composed of isotherm, isochore, and adiabat segments, em...This page discusses entropy as a state function that integrates to zero over circular paths returning to initial conditions. It examines a path composed of isotherm, isochore, and adiabat segments, emphasizing that although heat and work are path-dependent, entropy remains consistent. The analysis demonstrates that despite varying heat transfer values, the change in entropy remains the same, reinforcing its nature as a state function, in contrast to heat.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/03%3A_First_Law_of_Thermodynamics/3.02%3A_Work_and_HeatThe text discusses the contributions of James P. Joule to modern thermodynamics, particularly his experiments demonstrating that work and heat can both change a system's temperature, forming the basis...The text discusses the contributions of James P. Joule to modern thermodynamics, particularly his experiments demonstrating that work and heat can both change a system's temperature, forming the basis for the First Law of Thermodynamics. The law suggests that a system's capacity to do work is increased by heating or working on it, and it defines internal energy change as the sum of heat (q) and work (w).
- 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.
