For an ideal gas, it is. dH = dU + d(pV) = dU + RdT=(Cv+R)dTkelvin490 said:For an ideal gas, the internal energy is a function only of temperature, so that dU = CvdT can always be applied. I am not sure whether dH=CP dT is also always true even the pressure is not constant.
Internal energy is the total energy stored in a system, including the kinetic and potential energies of its particles.
An ideal gas is a theoretical gas that follows the gas laws at all pressures and temperatures, and whose particles have no volume or intermolecular forces.
The internal energy of an ideal gas is solely dependent on its temperature. This means that changes in pressure or volume will not affect the internal energy of an ideal gas.
The equation is dH = Cp * dT, where dH is the change in enthalpy, Cp is the specific heat at constant pressure, and dT is the change in temperature.
Yes, for an ideal gas, the change in enthalpy is always equal to the product of the specific heat at constant pressure and the change in temperature. This is because, as mentioned earlier, the internal energy of an ideal gas is solely dependent on its temperature.