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Ideal gases are assuming that gas particles are discrete point particles, thus bouncing off each other with no attraction with one another, and each molecule taking up no space. This assumption allows for the Ideal gas law, which states exact proportions between measurable quantities in gases: pressure, volume, temperature, number of particles.
The ideal gas law is: PV = nRT
where:
P is pressure
V is volume
n is number of moles of gas
R is ideal gas constant
T is temperature (K)
Real gases particles, as common sense suggest, do have volume and are minutely attracted to each other. Thus, gases do deviate from ideal behavior especially as they get more massive and voluminous. Thus, the attractions between the particles and the volume taken up by the particles must be taken into account. The equation derived by Van der Waals is the Van der Waals equation which simulates real gas behavior.
The Van der Waals equation is:
(p + ((n2a)/V2)(V - nb) = nRT
where:
p is measured pressure of the gas
n is number of moles of gas
a is attraction constant of the gas, varies from gas to gas
V is measured volume of the gas
b is volume constant of the gas, also varies from gas to gas
R is ideal gas constant
T is temperature (K)
Basically the Van der Waals equation is compensating for the non ideal attraction and volume of the gas. It is similar to PV = nRT, identical on the right side. To compensate for the massless volume that is found in ideal equation, the volume of the molecules are subtracted from the observed. Since, the equation of gas behavior concentrates on the space between the gas particles, and the volume of gas adds to the measured amount that should be used in the equation, thus it is subtracted from the equation. Another compensation is the fact that attraction between particles reduces the force on the walls of the container thus the pressure, thus it must be added back into the equation, thus the addition of the a term.
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What is the difference between the Ideal Gas Law and Kinetic Molecular Theory?
The Ideal Gas Law describes the behavior of ideal gases in terms of pressure, volume, temperature, and the number of gas particles. Kinetic Molecular Theory explains the behavior of gases in terms of the motion of gas particles and the interactions between them, helping to understand concepts such as temperature and pressure in relation to gas behavior.
Which of the following properties minimizes the differences between an ideal gas and a real gas?
- Weak intermolecular forces -Low density
What is the difference between ideal gas law and kinetic theory?
Ideal gas law is the law which states that for a given quantity of gas, the product of the volume V and pressure P is proportional to the absolute temperature T, or PV = kT, where k is a constant. And, kinetic theory of gas is the theory based on a simple description of a gas, from which many properties of gases can be derived.
What law was used to determine the relationship between the volume and the number of moles in this equation?
The ideal gas law: PV=nRT Where n=the number of moles
What is the difference between naturalist and romanticist?
If you mean as in the arts then here for example: naturalists paint a picture just like it is in the reality, but romanticists will paint it to be ideal, more beautiful.
Difference between Carnot and ideal cycle?
What is the difference between ideal and actual cycle?
Which of the following properties minimize the difference between an ideal gas and real gas?
low temperature, Strong intermolecular forces
What should be age difference between ideal couple for marriage?
The ideal age difference should be between 4 and 7.
What is the difference between an ideal and actual cycle?
fdfv tdfgd trvx
What is a major difference between folkways and mores?
The level to which the ideal is enforced
What is the difference between ideal and reciprocal altruism?
The difference between ideal and reciprocal altruism is in one, the person expects nothing in return. In reciprocal altruism, the person expects something back at some point.
What is the difference between the Ideal Gas Law and Kinetic Molecular Theory?
The Ideal Gas Law describes the behavior of ideal gases in terms of pressure, volume, temperature, and the number of gas particles. Kinetic Molecular Theory explains the behavior of gases in terms of the motion of gas particles and the interactions between them, helping to understand concepts such as temperature and pressure in relation to gas behavior.
What force causes a difference between the ideal and the actual mechanical advantage?
Friction is the main force that causes a difference between the ideal and actual mechanical advantage. Other factors like misalignment of the machine parts, wear and tear, and measurement inaccuracies can also contribute to this difference.
What force causes a difference between the ideal and the mechanical advantage Of the same object?
The force required to overcome friction between parts of a machine or device causes a difference between the ideal and mechanical advantage of the object. Friction reduces the efficiency of a machine by causing energy losses, making it harder to achieve the theoretical ideal advantage.
What is the difference between conveniently and convenience?
Conveniently is an adverb meaning in a way that is ideal or not difficult. A convenience is a noun meaning an ideal quality or situation.
What are the unique properties and uses of square crystals in the field of crystallography?
Square crystals have symmetrical properties that make them ideal for crystallography studies. Their uniform shape allows for precise measurements of angles and distances between atoms. In crystallography, square crystals are used to determine the atomic structure of materials, aiding in the development of new technologies and understanding of chemical properties.
What is the relationship between the internal energy of an ideal gas and its thermodynamic properties?
The internal energy of an ideal gas is directly related to its thermodynamic properties, such as temperature, pressure, and volume. Changes in these properties can affect the internal energy of the gas, and vice versa. The internal energy of an ideal gas is a measure of the total energy stored within the gas due to its molecular motion and interactions.
