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- https://chem.libretexts.org/Courses/can/CHEM_210%3A_General_Chemistry_I_(An_Atoms_Up_Approach)/15%3A_Gases_and_Gas_Laws/15.06%3A_Ideal_Gases_and_Real_GasesWe imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’...We imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’ law, and the ideal gas equation—and do so exactly. This is an oversimplification. In fact they are always approximations. They are approximately true for all gases under all “reasonable” conditions, but they are not exactly true for any real gas under any condition.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Book%3A_Introductory_Chemistry_Online_(Young)/09%3A_The_Gaseous_State/92%3A_The_Pressure-Volume_Relationship%3A_Boyles_LawBoyle found that the dependence of volume on pressure was non-linear but that a linear plot could be obtained if the volume was plotted against the reciprocal of the pressure, 1/P. The volume (V) of a...Boyle found that the dependence of volume on pressure was non-linear but that a linear plot could be obtained if the volume was plotted against the reciprocal of the pressure, 1/P. The volume (V) of an ideal gas varies inversely with the applied pressure (P) when the temperature (T) and the number of moles (n) of the gas are constant. The piston is adjusted so that the volume is 0.155 L and the pressure is 956 mm Hg; what was the initial volume?
- https://chem.libretexts.org/Courses/Western_Washington_University/Biophysical_Chemistry_(Smirnov_and_McCarty)/01%3A_Biochemical_Thermodynamics/1.02%3A_The_First_Law_of_ThermodynamicsSystems can undergo a change of state from some initial state to a final state accompanied by a change in the system???s energy. In this chapter, we analyze two types of energy: heat and work. This le...Systems can undergo a change of state from some initial state to a final state accompanied by a change in the system???s energy. In this chapter, we analyze two types of energy: heat and work. This leads to a presentation of the first law of thermodynamics that deals with the conservation of energy, stating that any changes in the total internal energy of the system must be due to exchanges of either heat or work with the surroundings.
- 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/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/19%3A_The_First_Law_of_ThermodynamicsThis page covers key concepts of classical thermodynamics, highlighting Joule's insights into work and heat, the distinction between state and path functions, and adiabatic processes. It explores the ...This page covers key concepts of classical thermodynamics, highlighting Joule's insights into work and heat, the distinction between state and path functions, and adiabatic processes. It explores the importance of enthalpy as a state function, its calculation using Hess's Law, and the role of temperature in thermodynamic functions, especially in isobaric processes.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Gases/Real_GasesIn the derivation of the ideal gas law, we assume that there are no attractive forces between the particles and that the particles don't take up any space. Since we know that attractive forces become ...In the derivation of the ideal gas law, we assume that there are no attractive forces between the particles and that the particles don't take up any space. Since we know that attractive forces become important at low temperatures, and that the volume of the particles will be important when the volume is relatively low (meaning pressure is high) we can predict that the ideal gas equation works best at high temperatures and low pressures.
- https://chem.libretexts.org/Courses/can/CHEM_210%3A_General_Chemistry_I_(An_Atoms_Up_Approach)/14%3A_Gases/14.03%3A_The_Ideal_Gas_Law/14.3.01%3A_Real_vs._Ideal_GasesWe imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’...We imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’ law, and the ideal gas equation—and do so exactly. This is an oversimplification. In fact they are always approximations. They are approximately true for all gases under all “reasonable” conditions, but they are not exactly true for any real gas under any condition.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/25%3A_Solutions_II_-_Nonvolatile_Solutes/25.02%3A_The_Activities_of_Nonvolatile_SolutesThis page explores fugacity and activity in non-ideal gases and solutions, emphasizing how fugacity represents effective pressure and activity measures a compound's behavior relative to standard condi...This page explores fugacity and activity in non-ideal gases and solutions, emphasizing how fugacity represents effective pressure and activity measures a compound's behavior relative to standard conditions. It explains the relationship between chemical potential and mole fraction through activity coefficients, crucial for calculating equilibrium constants. The text highlights the significance of a standardized reference state in chemistry as established by IUPAC.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Thermodynamics_and_Chemical_Equilibrium_(Ellgen)/02%3A_Gas_Laws/2.08%3A_Real_Gases_Versus_Ideal_GasesWe imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’...We imagine that the results of a large number of experiments are available for our analysis. Our characterization of these results has been that all gases obey the same equations—Boyle’s law, Charles’ law, and the ideal gas equation—and do so exactly. This is an oversimplification. In fact they are always approximations. They are approximately true for all gases under all “reasonable” conditions, but they are not exactly true for any real gas under any condition.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/07%3A_Mixtures_and_Solutions/7.01%3A_Thermodynamics_of_MixingThe document discusses the mixing of two ideal gases, beginning with their initial state in separate partitions of a container. Once mixed isothermally, partial pressures drop and volumes double, yet ...The document discusses the mixing of two ideal gases, beginning with their initial state in separate partitions of a container. Once mixed isothermally, partial pressures drop and volumes double, yet total pressure remains consistent. The enthalpy of mixing ΔHmix is zero due to ideal behavior, meaning no molecular interactions are considered. The entropy of mixing is positive since mixing increases disorder.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/09%3A_Chemical_Equilibria/9.02%3A_Chemical_PotentialThe page explains the concept of chemical equilibrium, focusing on how the chemical potential of reactants and products balance. Using the reaction A(g) ??? B(g), equilibrium is reached when chemical ...The page explains the concept of chemical equilibrium, focusing on how the chemical potential of reactants and products balance. Using the reaction A(g) ??? B(g), equilibrium is reached when chemical potentials equate. For ideal gases, this involves using mole fractions and equilibrium constants (K???). It discusses calculating the Gibbs free energy changes and their relation to K???, highlighting that ??G < 0 indicates a spontaneous reaction.
