What happens when a gas is expanded at constant temperature?

It is correct because at constant temperature kinetic energy of the gas remains the same. Therefore, if gas expands at a constant temperature the kinetic energy of the molecules remains the same. Kinetic energy of the gas is directly proportional to temperature of the gas.

What happens when an ideal gas expands?

As the volume of a gas expands, the overall temperature tends to drop because there are fewer molecules per any given volume. According to the ideal gas law PV=nRT, P=(n/V) RT, the pressure can be constant with decreasing molecular density only with increasing temperature.

When an ideal gas obeying kinetic theory of gases can be liquefied?

Ideal gas has no force of attraction and has negligible volume. Hence, it cannot be liquefied at any T and P.

When an ideal gas undergoes unrestrained expansion no cooling occurs because the molecules?

For an ideal gas, there is neither attraction nor repulsion since there are no intermolecular forces. Hence when an ideal gas undergoes unrestrained expansion no cooling occurs because the molecules exert no attractive forces on each other.

When an ideal gas expands in vacuum at a constant temperature then?

This process is called an expansion into a vacuum. As you described, the volume of the gas increases and the pressure drops, such that pV does not change at all. Since n is constant, T=pVnR is also constant.

What happens to temperature when gas is released?

So the atoms are “hotter” when they come away from the piston than they were before they struck it. Therefore all the atoms which are in the vessel will have picked up speed. This means that when we compress a gas slowly, the temperature of the gas increases.

Does ideal gas obey kinetic theory of gases?

Complete answer: In the question it is given that an ideal gas obeys kinetic theory of gases. According to the kinetic theory of gases, the gas molecules are very small compared to the distance between molecules.

How can ideal gas be liquefied?

Gases can be liquefied by lowering the temperature and increasing the pressure. An ideal gas have no intermolecular force of attraction, so it cannot be liquefied by applying high pressure and decreasing temperature.

When an ideal gas expands there is no cooling why?

When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules. When a non-ideal gas suddenly expands from a high pressure to a low pressure, there is a temperature change. This is called Joule-Thomson effect. It is an adiabatic effect.

What is the effect on temperature of an ideal gas when it undergoes a Joule Thomson adiabatic expansion?

zero
Joule’s second law It is easy to verify that for an ideal gas defined by suitable microscopic postulates that αT = 1, so the temperature change of such an ideal gas at a Joule–Thomson expansion is zero.

What happens when gas expands in vacuum?

Since the vacuum offers no resistance, the work is zero. In a vacuum,there is nothing that the gas can do work on! Also,there is nothing that the gas has to overcome its pressure to expand,so the work it does in expanding is zero.

When an ideal gas expands in vacuum no work done Why?

In an ideal gas, there are no intermolecular forces of attraction. Hence, no energy is required to overcome these forces,. Moreover, when a gas expands against vacuum,work done is zero( becausePext=0). Hence, internal energy of the system does not change,i.e., there is no absorption or evolution of heat.

What happens to the temperature when an ideal gas expands?

When an ideal gas expands then its temperature decreases because the frequency of atomic collisions decrease as gas expands, as a result the gas gets cooler.

What happens to heat when a gas is compressed?

As it does so, heat leaves / comes into the gas to keep the temperature constant. As the gas is compressed, the work done on it shows up as increased internal energy, which must be transferred to the surroundings to keep the temperature constant. At constant temperature, the gas law becomes

What happens to the kinetic energy of gas molecules during expansion?

Hence, at the constant temperature, the kinetic energy remains same. Thus during expansion of a gas at constant temperature, the kinetic energy of gas molecules remains same. Hence, option (B) is correct and option (C) is incorrect.

What happens to the enthalpy of an ideal gas during isenthalpic process?

Since the enthalpy of an ideal gas is a function of temperature only, during an isenthalpic process, the temperature of the ideal gas remains constant.