when pressure is applied on gas, it is covered to a liquid due to
a) increase in intermolecular forces of attraction between the particles
b) increase in intermolecular distances between the particles
c) decrease in intermolecular forces of attraction between the particles d) increase in kinetic energy of particles
Answers
Answer:
The particles of a real gas do, in fact, occupy a finite, measurable volume. At high pressures, the deviation from ideal behavior occurs because the finite volume that the gas molecules occupy is significant compared to the total volume of the container. The van der Waals equation modifies the ideal gas law to correct for this excluded volume, and is written as follows:
P
(
V
−
n
b
)
=
n
R
T
The available volume is now represented as
V
−
n
b
, where b is a constant that is specific to each gas. In this approximation, the gas molecules are considered hard spheres with a defined radius (r) that cannot overlap with the radius of a neighboring particle. The constant b is defined as:
b
=
4
N
A
⋅
4
3
π
⋅
r
3
where NA is Avogadro’s number and r is the radius of the molecule.
It is important to note that this equation applies to ideal gases as well. It can be simplified because in an ideal situation, the value of b is so much smaller than V that it does not make a measurable difference in the calculation.
Explanation:
The particles of a real gas do, in fact, occupy a finite, measurable volume. At high pressures, the deviation from ideal behavior occurs because the finite volume that the gas molecules occupy is significant compared to the total volume of the container. The van der Waals equation modifies the ideal gas law to correct for this excluded volume, and is written as follows:
P
(
V
−
n
b
)
=
n
R
T
The available volume is now represented as
V
−
n
b
, where b is a constant that is specific to each gas. In this approximation, the gas molecules are considered hard spheres with a defined radius (r) that cannot overlap with the radius of a neighboring particle. The constant b is defined as:
b
=
4
N
A
⋅
4
3
π
⋅
r
3
where NA is Avogadro’s number and r is the radius of the molecule.
It is important to note that this equation applies to ideal gases as well. It can be simplified because in an ideal situation, the value of b is so much smaller than V that it does not make a measurable difference in the calculation.