Question

A real gas behaves least like an ideal gas under the conditions of

Answer 1

Answer: Option (2) is the correct answer.

Explanation:

A real gas behaves least like an ideal gas under the conditions of low temperature and high pressure.

This is because at low temperature and high pressure molecules of gas will have negligible kinetic energy and strong force of attraction. Thus, real gas will not behave like an ideal gas.

Whereas at high temperature and low pressure a real gas will behave like an ideal gas.

Answer 2

A real gas behaves least like an ideal gas under the conditions of $\boxed{{\text{(2) low temperature and high pressure}}}$ .

Further Explanation:

An ideal gas is a hypothetical gas that is composed of a large number of randomly moving particles that are supposed to have perfectly elastic collisions among themselves. It is just a theoretical concept and practically no such gas exists. But gases tend to behave almost ideally at a higher temperature and lower pressure.

The expression for the ideal gas equation of gas is as follows:

$PV = nRT$                                                                            …… (1)

Here,

P is the pressure of the gas.

V is the volume of gas.

T is the absolute temperature of gas.

n denotes the number of moles of gas.

R is the universal gas constant.

Real gas:

It is also known as non-ideal gas as it shows deviations from its ideal behavior. This is because of the interactions between the molecules. There exist intermolecular forces between the gas molecules that are absent in ideal gas. The behavior of ideal gases is studied by van der Waals equation, that is expressed as follows:

$\left({P+\frac{{a{n^2}}}{{{V^2}}}}\right)\left({V-nb}\right)=nRT$                                                      …… (2)

Here,

P is the pressure of real gas.

V is the volume of real gas.

T is the absolute temperature of real gas.

n is the number of moles of real gas.

R is the universal gas constant.

a and b are the constants for real gas.

At high temperature and low pressure, energy due to intermolecular forces becomes less important in comparison to the kinetic energy of particles. The size of molecules also becomes less significant than the empty space between the gas molecules. So real gases behave in a similar manner to ideal gases at high temperature and low pressure.

But at low temperature and high pressure, the kinetic energy of gas molecules is negligible and molecules will have negligible forces of attraction. So real gases will behave least like an ideal gas under such conditions.

Learn more:

1. Which statement is true for Boyle’s law: brainly.com/question/1158880

2. Calculation of volume of gas: brainly.com/question/3636135

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Ideal gas equation

Keywords: ideal gas, pressure, volume, absolute temperature, equation of state, hypothetical, universal gas constant, real gas, high temperature, low temperature, high pressure, low pressure.