Question

In an isothermal process the internal energy of gas molecules decreases? Why?

Answer 1

Explanation:

the isothermal compression of a gas there is work done on the system to decrease the volume and increase the pressure. Doing work on the gas increases the internal energy and will tend to increase the temperature. To maintain the constant temperature energy must leave the system as heat and enter the environment.

Answer 2

Answer:

• A gas's isothermal compression is the system is being worked on to reduce volume and increase pressure.
• Working on the gas increases its internal energy and tends to raise its temperature. To keep the temperature constant, energy must leave the system as heat and enter the environment.

• A thermodynamic process in which the temperature of a system remains constant is known as an isothermal process. Heat is transferred into and out of the system at such a slow rate that thermal equilibrium is maintained.
• An ideal gas's internal energy is only a function of absolute temperature. Because there is no change in temperature in an isothermal process, the change in internal energy is also zero. As a result, the system's internal energy remains constant.
• The temperature remains constant in an isothermal process. As a result, internal energy remains constant, with a net change in internal energy of ZERO.

• Because an ideal gas has no particle interactions and no intermolecular forces, pressure changes at constant temperature have no effect on internal energy.

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