Which of the following statements concerning real gases is/are correct? (1) Nonideality in gas behavior becomes more pronounced as the pressure of a gas is decreased. (2) Nonideality in gas behavior becomes more pronounced as the temperature of a gas is decreased. (3) The measured pressure of a container of chlorine gas is generally lower than the pressure calculated by the ideal gas law.

The statements concerning real gases that are correct include:

2. Nonideality in gas behavior becomes more pronounced as the temperature of a gas is decreased.

3. The measured pressure of a container of chlorine gas is generally lower than the pressure calculated by the ideal gas law.

A real gas is also referred to as a non-ideal gas and it can be defined as a gas that do not behave as an ideal gas at all standard pressure and temperature (STP) conditions, due to interactions between its molecules. Thus, a real gas does not obey the ideal gas law.

Some of the characteristics of a real gas are:

Hence, the measured pressure of a container of chlorine gas is generally lower than the pressure when calculated by using the ideal gas law equation. Also, nonideality in gas behavior becomes evident as the temperature of a gas is decreased.

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Nonideality in gas behavior becomes more pronounced as the temperature of a gas is decreased.

The measured pressure of a container of chlorine gas is generally lower than the pressure calculated by the ideal gas law

Explanation:

Gases are said to show ideal behavior at low pressure and high temperature. Recall that the kinetic theory of gases assumes a zero intermolecular force of attraction between gas molecules. Hence it is assumed that gas molecules are infinitely free and move about at high velocities. The gas molecules are believed not to interact with each other in any way.

However, at lower temperature, gas molecules deviate from ideal behaviour and significant intermolecular interaction is observed. This implies that gases tend towards non ideality at lower temperatures.

Also, the assumption that gas molecules do not interact with each whatsoever has been found not to be completely true as there is some degree of intermolecular interaction between the molecules of real gases. The implication of this is that the measured pressure of real gases is less than the pressure calculated on the basis of the ideal gas equation.

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explanation:

1. they vary with a higher number because boiling is way hotter than melting