What are the differences between ideal gas and real gas?

Answer 1

The difference between an ideal gas and a real gas is that real gases will not strictly follow the laws established for ideal gases, because of real-world characteristics.

An ideal gas can follow the formula PV=nRT

(P - pressure, V - volume, n - amount of moles, R - Avogrado constant, T - absolute temperature)

A real gas does not always follow this formula.

• An ideal gas is infinitely compressible, a real gas will condense to a liquid at some pressure.
• The particles of an ideal gas lose no energy to its container. A real gas conducts and radiates heat, thereby losing energy.
• There is no attraction between the molecules of an ideal gas. A real gas has particle attractions.

Answer 2

An ideal gas is basically an imaginary substance which:

Acts as a point particle - i.e. each atom/molecule of gas is treated as a dimensionless moving point in space rather then having a geometric shape.

The molecules do not interact with each other in any way other then translation of momentum.

These assumptions work for most gases at standard temperature and pressure due to the fact that the relative distances between each gas particle is large enough to negate electrostatic attractions, and when the particles come in contact with one another their velocities overcome said attractions.

Real gases, in reality do have dimensions larger then zero and do interact electrostatically, but as stated above these realities can be ignored in high school and even undergraduate university.

Answer 3

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, dohave 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 Vander Waals is the Vander Waals equation which simulates real gas behavior.

The Vander 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 Vander 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 mass less 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.

Answer 4

ideal gases are gases that are stable.they are in the last group of the Periodic Table.they are aalso known as the rare gases,noble gases,e.t.c.they are different from other gases because they are stable which makes other gases that try to be stable.

Answer 5

For the sake of easy math, we make several assumptions for an ideal gas: 1. the gas particles themselves have no volume, 2. the collisions between gas particles are 100% elastic, and 3. the gas particles do not interact with each other in any way. All three of these assumptions are false, however, because all matter has volume, no collisions are completely elastic, and there is some type of inter-particle attraction with any gas. But it makes the math easier, and we can now use the same equation (PV=nRT) for all gases. It's close enough that it usually works. The conditions under which real gases most closely resemble an ideal gas is low pressure and high temperature. The conditions under which real gases deviate the most from ideal gas behavior is high pressure and low temperature.

Answer 6

Ideal gases follow the ideal gas law exactly, while real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces. Real gases have volume and experience attractive and repulsive forces among molecules, whereas ideal gases are assumed to have no volume and no intermolecular forces.

Answer 7

Real gases are those that do not obey the gas laws. Ideal gases do.

Answer 8

Two main differences - ideal gases lack intermolecular forces, and ideal gases are composed of molecules that themselves take up no volume. Neither of these statements are true of real gases.

Answer 9

Real gas or perfect gas has comparasion factor(z) equal to one