The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to;
430 J = 120 J + (internal energy change)
so
Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
In an adiabatic process, the work done is equal to the change in internal energy of a system.
Delta "u" typically stands for change in internal energy in thermodynamics. It represents the difference between the final internal energy of a system and its initial internal energy. It is often used to calculate the heat and work interactions in a thermodynamic process.
In an isothermal process, the internal energy of a system remains constant because the temperature does not change. This means that the relationship between internal energy and temperature is that they are directly proportional in an isothermal process.
The work done by an expanding gas is directly related to the change in its internal energy. When a gas expands, it does work on its surroundings, which can lead to a change in its internal energy. This change in internal energy is a result of the work done by the gas during the expansion process.
In an adiabatic process, where there is no heat exchange with the surroundings, the change in internal energy is equal to the negative of the work done. This relationship is a result of the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
In an adiabatic process, the work done is equal to the change in internal energy of a system.
The process is known as an isothermal process. In an isothermal process, the energy transferred to the gas as heat and work results in no change in the gas's internal energy because the temperature remains constant throughout the process.
Delta "u" typically stands for change in internal energy in thermodynamics. It represents the difference between the final internal energy of a system and its initial internal energy. It is often used to calculate the heat and work interactions in a thermodynamic process.
In an isothermal process, the internal energy of a system remains constant because the temperature does not change. This means that the relationship between internal energy and temperature is that they are directly proportional in an isothermal process.
The work done by an expanding gas is directly related to the change in its internal energy. When a gas expands, it does work on its surroundings, which can lead to a change in its internal energy. This change in internal energy is a result of the work done by the gas during the expansion process.
In an adiabatic process, where there is no heat exchange with the surroundings, the change in internal energy is equal to the negative of the work done. This relationship is a result of the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system.
The change would be 100 joules, because an isochoric system can not perform the work.
In an isochoric (constant volume) process, there is no change in volume, so the work done is zero. Therefore, all the heat added goes into increasing the internal energy of the system. The change in internal energy of the gas would be equal to the heat added, which in this case is 400 J.
Since internal energy is a state function and a cyclic process always returns to the same state (that's how you define a cyclic process), the value of the the internal energy will remain constant. That is not to say that it doesn't change along the cyclic path during the process - just that it always returns to the same value when the cycle is complete.
The entropy of an ideal gas during an isothermal process may change because normally the entropy is a net zero. The change of on isothermal process can produce positive energy.
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.
In an adiabatic process, no heat is exchanged with the surroundings. The work done is the change in internal energy of the system, which is equal to the pressure times the change in volume.