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What is the difference between delta H and delta E in thermodynamics?
In thermodynamics, delta H represents the change in enthalpy, which is the heat energy exchanged during a process at constant pressure. Delta E, on the other hand, represents the change in internal energy, which is the total energy of a system. Enthalpy includes both internal energy and the energy required to change the system's volume, while internal energy only considers the system's total energy.
What is the difference between enthalpy and heat, and how do they relate to each other in the context of thermodynamics?
Enthalpy is a measure of the total energy in a system, including both internal energy and pressure-volume work. Heat, on the other hand, is the transfer of energy between a system and its surroundings due to a temperature difference. In thermodynamics, enthalpy change is related to heat transfer at constant pressure through the equation H q PV, where q is the heat transferred and PV is the pressure-volume work done by the system.
What are the units for Gibbs free energy and how are they determined in thermodynamics?
The units for Gibbs free energy are joules (J) or kilojoules (kJ). In thermodynamics, Gibbs free energy is determined by calculating the difference between the enthalpy (H) and the product of the temperature (T) and the entropy (S), using the equation: G H - TS.
What is the relationship between adiabatic processes and the change in enthalpy (H)?
In adiabatic processes, there is no heat exchange with the surroundings, so the change in enthalpy (H) is equal to the change in internal energy (U). This means that in adiabatic processes, the change in enthalpy is solely determined by the change in internal energy.
What is the difference between the enthalpy of the products and the enthalpy of the reactants in a chemical reaction?
The difference between the enthalpy of the products and the enthalpy of the reactants in a chemical reaction is known as the change in enthalpy, or H. This value represents the amount of heat energy either absorbed or released during the reaction. If H is positive, the reaction is endothermic and absorbs heat. If H is negative, the reaction is exothermic and releases heat.
What is the difference between delta H and delta E in thermodynamics?
In thermodynamics, delta H represents the change in enthalpy, which is the heat energy exchanged during a process at constant pressure. Delta E, on the other hand, represents the change in internal energy, which is the total energy of a system. Enthalpy includes both internal energy and the energy required to change the system's volume, while internal energy only considers the system's total energy.
What is the difference between enthalpy and heat, and how do they relate to each other in the context of thermodynamics?
Enthalpy is a measure of the total energy in a system, including both internal energy and pressure-volume work. Heat, on the other hand, is the transfer of energy between a system and its surroundings due to a temperature difference. In thermodynamics, enthalpy change is related to heat transfer at constant pressure through the equation H q PV, where q is the heat transferred and PV is the pressure-volume work done by the system.
What is the difference between internal energy and enthalpy?
Internal energy is the total energy stored within a system, including the energy associated with the motion and interactions of its particles. Enthalpy, on the other hand, is the total heat content of a system at constant pressure, including the internal energy and the energy required to displace the surroundings.
What is the difference between the Gibbs and Helmholtz free energy equations and how do they relate to each other in thermodynamics?
The Gibbs free energy equation considers both the enthalpy and entropy of a system, while the Helmholtz free energy equation only considers the internal energy and entropy. In thermodynamics, these equations are related through the relationship G H - TS, where G is the change in Gibbs free energy, H is the change in enthalpy, S is the change in entropy, and T is the temperature. This equation helps determine whether a reaction is spontaneous or non-spontaneous at a given temperature.
What are the units for Gibbs free energy and how are they determined in thermodynamics?
The units for Gibbs free energy are joules (J) or kilojoules (kJ). In thermodynamics, Gibbs free energy is determined by calculating the difference between the enthalpy (H) and the product of the temperature (T) and the entropy (S), using the equation: G H - TS.
What is the relationship between adiabatic processes and the change in enthalpy (H)?
In adiabatic processes, there is no heat exchange with the surroundings, so the change in enthalpy (H) is equal to the change in internal energy (U). This means that in adiabatic processes, the change in enthalpy is solely determined by the change in internal energy.
What is a difference between ionisation enthalpy and electron gain enthalpy?
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What is the difference between the enthalpy of the products and the enthalpy of the reactants in a chemical reaction?
The difference between the enthalpy of the products and the enthalpy of the reactants in a chemical reaction is known as the change in enthalpy, or H. This value represents the amount of heat energy either absorbed or released during the reaction. If H is positive, the reaction is endothermic and absorbs heat. If H is negative, the reaction is exothermic and releases heat.
What is the difference between external and internal communications?
What is the difference between external and internal communications
What is the difference between external and internal indicator?
what is the difference between the external & internal indicator
What is Difference between internal and external indicators?
what is the difference between the external & internal indicator
How is Hf related to the H of a reaction?
The Hreaction is the difference between Hf, products and Hf, reactants
