Question

В ходе адиабатного процесса внутренней энергии один моль разряжена гелия увеличивается как изменяется при этом температура гелия и его давление

Answer 1

Если процесс адиабатный то внутренняя энергия может увеличиться за счет работы внешних сил ( адиабатное сжатие)


при адиабатном сжатии температура газа увеличивается

Answer 2

Adiabatic Process and Change in Internal Energy, Temperature, and Pressure of Helium

During an adiabatic process, the internal energy of one mole of helium decreases as the temperature and pressure of the helium change. The specific relationship between these variables can be described by the adiabatic equation:

T = T0 * (V/V0)^(γ-1)

Where: - T is the final temperature of the helium - T0 is the initial temperature of the helium - V is the final volume of the helium - V0 is the initial volume of the helium - γ is the heat capacity ratio or adiabatic index, which is a constant value for a specific gas

The adiabatic equation shows that as the volume of helium increases (V > V0), the temperature of the helium decreases (T < T0). Conversely, if the volume of helium decreases (V < V0), the temperature of the helium increases (T > T0).

It's important to note that the adiabatic process assumes no heat exchange with the surroundings. This means that the process occurs without any transfer of heat energy between the helium and its surroundings. As a result, the change in internal energy is solely due to the work done on or by the helium gas.

The pressure of the helium during an adiabatic process can also be determined using the adiabatic equation and the ideal gas law:

P = P0 * (V/V0)^γ

Where: - P is the final pressure of the helium - P0 is the initial pressure of the helium

The adiabatic equation for pressure shows that as the volume of helium increases (V > V0), the pressure of the helium decreases (P < P0). Conversely, if the volume of helium decreases (V < V0), the pressure of the helium increases (P > P0).

It's important to note that the adiabatic process assumes that the helium gas behaves ideally, following the ideal gas law. This means that the gas particles are assumed to be point masses with no intermolecular forces and occupy negligible volume compared to the total volume of the gas.

In summary, during an adiabatic process, the internal energy of one mole of helium decreases as the temperature and pressure of the helium change. The specific relationship between these variables is described by the adiabatic equation, which shows that as the volume of helium increases, the temperature and pressure of the helium decrease, and vice versa