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The difference between heat and internal energy is that heat is technically a process by which energy is transferred between systems and internal energy is actual total energy of a system.
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The meaning and use of terms related heat, temperature, energy varies depending on whether one is informally describing thermodynamic processes or one is being rigorous according to the definitions of thermodynamiocs. For most communication, even most scientific communication, the informal understandings are adequate.
The nuances of the technical terms requires the study of thermodynamics, but will be (too) briefly described below.
- Temperature is directly proportional to the amount of kinetic energy the individual particles have within a body.
- Internal energy of a system is the total energy of the system. It is the sum of the potential and kinetic energies in all forms, including chemical bonds, rest mass, magnetic energy and everything else.
- Heat is thermal energy transferred to body. It is energy transferred through a temperature difference. Cold objects gain heat from warm ones.
- Thermal energy is energy associated with temperature. Thermal energy is not kinetic energy or heat. It is not a rigorously defined thermodynamic quantity when taken out of context.
- Work is force times distance, a mechanical process which changes the total energy of a system and does not require heat.
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What is the difference between enthalpy and internal energy in thermodynamics?
Enthalpy is the total heat content of a system at constant pressure, including internal energy and the energy required to displace the surroundings. Internal energy is the total energy stored within a system, including kinetic and potential energy of its particles.
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 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 bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction?
The difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction represents the energy change that occurs during the reaction. If the bond enthalpy of the products is lower than that of the reactants, it indicates that energy is released during the reaction, making it exothermic. Conversely, if the bond enthalpy of the products is higher than that of the reactants, it indicates that energy is absorbed during the reaction, making it endothermic.
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 enthalpy and internal energy in thermodynamics?
Enthalpy is the total heat content of a system at constant pressure, including internal energy and the energy required to displace the surroundings. Internal energy is the total energy stored within a system, including kinetic and potential energy of its particles.
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 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 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.
How can the enthalpy of air be calculated?
The enthalpy of air can be calculated using the equation: enthalpy internal energy pressure volume. This equation takes into account the internal energy of the air and the pressure and volume of the system.
Internal energy and enthalpy how differ and relate to each other?
Enthalpy mathematically is the sum of the internal energy and work done in a process.internal energy is the sum of the kinetic energy,potential energy,vibrational energies etc
What is the difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction?
The difference between the bond enthalpy of the reactants and the bond enthalpy of the products in a chemical reaction represents the energy change that occurs during the reaction. If the bond enthalpy of the products is lower than that of the reactants, it indicates that energy is released during the reaction, making it exothermic. Conversely, if the bond enthalpy of the products is higher than that of the reactants, it indicates that energy is absorbed during the reaction, making it endothermic.
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.
When should one choose to use internal energy or enthalpy in a thermodynamic analysis?
One should choose to use internal energy when focusing on the system's energy changes, and enthalpy when considering heat transfer at constant pressure.
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 enthalpy change and enthalpy change per mole?
Enthalpy is the energy absorbed or lost from a reaction, but enthalpy change per mole is the amount of energy lost per mole, so in order to get the overall enthalpy from the change per mole, you must multiply that value by the amount of moles used in the reaction.
How can the relationship between enthalpy change (H), internal energy change (U), and pressure-volume work change ((PV)) be expressed in a single equation?
The relationship between enthalpy change (H), internal energy change (U), and pressure-volume work change ((PV)) can be expressed in a single equation as: H U (PV).
