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Energy of formation is a http://www.answers.com/topic/thermodynamic-potential which measures the "useful" or process-initiating work obtainable from an http://www.answers.com/topic/isothermal-process, http://www.answers.com/topic/isobaric-process http://www.answers.com/topic/thermodynamic-system-1. Technically, the Gibbs free energy is the maximum amount of non-expansion work which can be extracted from a http://www.answers.com/topic/closed-system or this maximum can be attained only in a completely http://www.answers.com/topic/reversibility-3. When a system changes from a well-defined initial state to a well-defined final state, the Gibbs free energy ΔG equals the work exchanged by the system with its surroundings, less the work of the pressure forces, during a reversible transformation of the system from the same initial state to the same final state. Gibbs energy is also the chemical potential that is minimized when a system reaches equilibrium at constant pressure and temperature. As such, it is a convenient criterion of spontaneity for processes with constant pressure and temperature. The Gibbs free energy, originally called available energy, was developed in the 1870s by the American mathematical physicist http://www.answers.com/topic/willard-gibbs. In 1873, in a footnote, Gibbs defined what he called the "available energy" of a body as such: "The greatest amount of http://www.answers.com/topic/work-physics-in-encyclopedia which can be obtained from a given quantity of a certain substance in a given initial state, without increasing its total http://www.answers.com/topic/volume or allowing http://www.answers.com/topic/heat to pass to or from external bodies, except such as at the close of the processes are left in their initial condition." The initial state of the body, according to Gibbs, is supposed to be such that "the body can be made to pass from it to states of http://www.answers.com/topic/friction-1 by http://www.answers.com/topic/reversibility-3". In his 1876 http://www.answers.com/topic/magnum-opus http://www.answers.com/topic/on-the-equilibrium-of-heterogeneous-substances, a graphical analysis of multi-phase chemical systems, he engaged his thoughts on chemical free energy in full. Energy of formation is a http://www.answers.com/topic/thermodynamic-potential which measures the "useful" or process-initiating work obtainable from an http://www.answers.com/topic/isothermal-process, http://www.answers.com/topic/isobaric-process http://www.answers.com/topic/thermodynamic-system-1. Technically, the Gibbs free energy is the maximum amount of non-expansion work which can be extracted from a http://www.answers.com/topic/closed-system or this maximum can be attained only in a completely http://www.answers.com/topic/reversibility-3. When a system changes from a well-defined initial state to a well-defined final state, the Gibbs free energy ΔG equals the work exchanged by the system with its surroundings, less the work of the pressure forces, during a reversible transformation of the system from the same initial state to the same final state. Gibbs energy is also the chemical potential that is minimized when a system reaches equilibrium at constant pressure and temperature. As such, it is a convenient criterion of spontaneity for processes with constant pressure and temperature. The Gibbs free energy, originally called available energy, was developed in the 1870s by the American mathematical physicist http://www.answers.com/topic/willard-gibbs. In 1873, in a footnote, Gibbs defined what he called the "available energy" of a body as such: "The greatest amount of http://www.answers.com/topic/work-physics-in-encyclopedia which can be obtained from a given quantity of a certain substance in a given initial state, without increasing its total http://www.answers.com/topic/volume or allowing http://www.answers.com/topic/heat to pass to or from external bodies, except such as at the close of the processes are left in their initial condition." The initial state of the body, according to Gibbs, is supposed to be such that "the body can be made to pass from it to states of http://www.answers.com/topic/friction-1 by http://www.answers.com/topic/reversibility-3". In his 1876 http://www.answers.com/topic/magnum-opus http://www.answers.com/topic/on-the-equilibrium-of-heterogeneous-substances, a graphical analysis of multi-phase chemical systems, he engaged his thoughts on chemical free energy in full. Energy of formation is a http://www.answers.com/topic/thermodynamic-potential which measures the "useful" or process-initiating work obtainable from an http://www.answers.com/topic/isothermal-process, http://www.answers.com/topic/isobaric-process http://www.answers.com/topic/thermodynamic-system-1. Technically, the Gibbs free energy is the maximum amount of non-expansion work which can be extracted from a http://www.answers.com/topic/closed-system or this maximum can be attained only in a completely http://www.answers.com/topic/reversibility-3. When a system changes from a well-defined initial state to a well-defined final state, the Gibbs free energy ΔG equals the work exchanged by the system with its surroundings, less the work of the pressure forces, during a reversible transformation of the system from the same initial state to the same final state. Gibbs energy is also the chemical potential that is minimized when a system reaches equilibrium at constant pressure and temperature. As such, it is a convenient criterion of spontaneity for processes with constant pressure and temperature. The Gibbs free energy, originally called available energy, was developed in the 1870s by the American mathematical physicist http://www.answers.com/topic/willard-gibbs. In 1873, in a footnote, Gibbs defined what he called the "available energy" of a body as such: "The greatest amount of http://www.answers.com/topic/work-physics-in-encyclopedia which can be obtained from a given quantity of a certain substance in a given initial state, without increasing its total http://www.answers.com/topic/volume or allowing http://www.answers.com/topic/heat to pass to or from external bodies, except such as at the close of the processes are left in their initial condition." The initial state of the body, according to Gibbs, is supposed to be such that "the body can be made to pass from it to states of http://www.answers.com/topic/friction-1 by http://www.answers.com/topic/reversibility-3". In his 1876 http://www.answers.com/topic/magnum-opus http://www.answers.com/topic/on-the-equilibrium-of-heterogeneous-substances, a graphical analysis of multi-phase chemical systems, he engaged his thoughts on chemical free energy in full. Energy of formation is a http://www.answers.com/topic/thermodynamic-potential which measures the "useful" or process-initiating work obtainable from an http://www.answers.com/topic/isothermal-process, http://www.answers.com/topic/isobaric-process http://www.answers.com/topic/thermodynamic-system-1. Technically, the Gibbs free energy is the maximum amount of non-expansion work which can be extracted from a http://www.answers.com/topic/closed-system or this maximum can be attained only in a completely http://www.answers.com/topic/reversibility-3. When a system changes from a well-defined initial state to a well-defined final state, the Gibbs free energy ΔG equals the work exchanged by the system with its surroundings, less the work of the pressure forces, during a reversible transformation of the system from the same initial state to the same final state. Gibbs energy is also the chemical potential that is minimized when a system reaches equilibrium at constant pressure and temperature. As such, it is a convenient criterion of spontaneity for processes with constant pressure and temperature. The Gibbs free energy, originally called available energy, was developed in the 1870s by the American mathematical physicist http://www.answers.com/topic/willard-gibbs. In 1873, in a footnote, Gibbs defined what he called the "available energy" of a body as such: "The greatest amount of http://www.answers.com/topic/work-physics-in-encyclopedia which can be obtained from a given quantity of a certain substance in a given initial state, without increasing its total http://www.answers.com/topic/volume or allowing http://www.answers.com/topic/heat to pass to or from external bodies, except such as at the close of the processes are left in their initial condition." The initial state of the body, according to Gibbs, is supposed to be such that "the body can be made to pass from it to states of http://www.answers.com/topic/friction-1 by http://www.answers.com/topic/reversibility-3". In his 1876 http://www.answers.com/topic/magnum-opus http://www.answers.com/topic/on-the-equilibrium-of-heterogeneous-substances, a graphical analysis of multi-phase chemical systems, he engaged his thoughts on chemical free energy in full.
What else can I help you with?
What is the free energy for ammonium oxalate?
The free energy for a compound like ammonium oxalate would depend on the specific conditions of the system, such as temperature and pressure. The free energy can be calculated using the Gibbs free energy equation, which takes into account the enthalpy and entropy changes of the reaction. You would need specific experimental data or calculations to determine the free energy for ammonium oxalate under particular conditions.
What is the relationship between the standard free energies of formation and the thermodynamic stability of a chemical compound?
The standard free energy of formation indicates the stability of a chemical compound. A lower value suggests greater thermodynamic stability, meaning the compound is more likely to form and exist in a given environment.
What is the difference between Gibbs free energy and standard free energy, and how do they relate to each other in chemical reactions?
Gibbs free energy and standard free energy are both measures of the energy available to do work in a chemical reaction. The main difference is that Gibbs free energy takes into account the temperature and pressure of the system, while standard free energy is measured under specific standard conditions. In chemical reactions, the change in Gibbs free energy determines whether a reaction is spontaneous or non-spontaneous. If the Gibbs free energy change is negative, the reaction is spontaneous, while a positive change indicates a non-spontaneous reaction. The relationship between Gibbs free energy and standard free energy lies in the fact that the standard free energy change can be used to calculate the Gibbs free energy change under any conditions.
What is the relationship between the standard Gibbs free energy change (G) and the actual Gibbs free energy change (G) in a chemical reaction?
The relationship between the standard Gibbs free energy change (G) and the actual Gibbs free energy change (G) in a chemical reaction is that the standard Gibbs free energy change is the value calculated under standard conditions, while the actual Gibbs free energy change takes into account the specific conditions of the reaction. The actual Gibbs free energy change can be different from the standard value depending on factors such as temperature, pressure, and concentrations of reactants and products.
What are the units for standard Gibbs free energy?
The units for standard Gibbs free energy are joules per mole (J/mol) or kilojoules per mole (kJ/mol).
What is the free energy for ammonium oxalate?
The free energy for a compound like ammonium oxalate would depend on the specific conditions of the system, such as temperature and pressure. The free energy can be calculated using the Gibbs free energy equation, which takes into account the enthalpy and entropy changes of the reaction. You would need specific experimental data or calculations to determine the free energy for ammonium oxalate under particular conditions.
What is the standard heat of formation of a free element in its standard state?
The standard heat of formation of a free element in its standard state is defined as zero. This is because it is the reference point from which the heat of formation of other compounds is determined.
What is the relationship between the standard free energies of formation and the thermodynamic stability of a chemical compound?
The standard free energy of formation indicates the stability of a chemical compound. A lower value suggests greater thermodynamic stability, meaning the compound is more likely to form and exist in a given environment.
What is the difference between Gibbs free energy and standard free energy, and how do they relate to each other in chemical reactions?
Gibbs free energy and standard free energy are both measures of the energy available to do work in a chemical reaction. The main difference is that Gibbs free energy takes into account the temperature and pressure of the system, while standard free energy is measured under specific standard conditions. In chemical reactions, the change in Gibbs free energy determines whether a reaction is spontaneous or non-spontaneous. If the Gibbs free energy change is negative, the reaction is spontaneous, while a positive change indicates a non-spontaneous reaction. The relationship between Gibbs free energy and standard free energy lies in the fact that the standard free energy change can be used to calculate the Gibbs free energy change under any conditions.
What is the free energy for C2O4-2?
The free energy for the C2O4-2 ion can vary depending on the specific conditions such as temperature and pressure. To calculate the free energy for C2O4-2, you would typically need to know the free energy of formation for the ion under standard conditions and apply appropriate corrections based on the specific conditions of interest.
What information can you provide about the delta gf table?
The delta Gf table provides information about the standard Gibbs free energy of formation for various compounds. This value indicates the stability of a compound relative to its elements in their standard states.
What is the relationship between the standard Gibbs free energy change (G) and the actual Gibbs free energy change (G) in a chemical reaction?
The relationship between the standard Gibbs free energy change (G) and the actual Gibbs free energy change (G) in a chemical reaction is that the standard Gibbs free energy change is the value calculated under standard conditions, while the actual Gibbs free energy change takes into account the specific conditions of the reaction. The actual Gibbs free energy change can be different from the standard value depending on factors such as temperature, pressure, and concentrations of reactants and products.
What are the units for standard Gibbs free energy?
The units for standard Gibbs free energy are joules per mole (J/mol) or kilojoules per mole (kJ/mol).
Is C2H2 plus H2 equal C2H4 spontenous written?
The standard free energy of formation of C2H2 is +209.20 kJ/mole, while that of C2H4 is +68.15 kJ/mole (and H2 zero since it is an element in its standard state). thus, at standard temperature and pressure (25 C, 1 Bar pressure) the reaction C2H2 + H2 -> C2H4 has a standard free energy change of -141 kJ/mole and thus "spontaneous" in that equilibrium constant >> 1.
What is Gibbs Free energy?
The usable energy released or absorbed by a reaction.
What is the G for the following reaction under standard conditions (T 298 K) for the formation of NH4NO3(s)?
To determine the Gibbs free energy change (ΔG°) for the formation of NH4NO3(s) under standard conditions (298 K), you would typically refer to standard Gibbs free energy of formation values for the reactants and products involved in the reaction. The reaction is: [ \text{N}_2(g) + 2 \text{H}_2(g) + \text{O}_2(g) \rightarrow \text{NH}_4\text{NO}_3(s) ] By using the standard Gibbs free energies of formation (ΔGf°) for the reactants and products, you can calculate ΔG° using the equation: [ ΔG° = Σ(ΔGf° \text{ of products}) - Σ(ΔGf° \text{ of reactants}) ] Without the specific values, I cannot provide a numerical answer, but this is the method you would use to find ΔG° for the reaction.
What is the standard free energy equation and how is it used to calculate the thermodynamic feasibility of a chemical reaction?
The standard free energy equation is G H - TS, where G is the standard free energy change, H is the standard enthalpy change, T is the temperature in Kelvin, and S is the standard entropy change. This equation is used to calculate the thermodynamic feasibility of a chemical reaction by comparing the standard free energy change to zero. If G is negative, the reaction is thermodynamically feasible and will proceed spontaneously. If G is positive, the reaction is not thermodynamically feasible and will not proceed spontaneously.
