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Gases summary

summary of general chemistry
Module

General and Organic Chemistry (AOC106DI)

26 Documents
Students shared 26 documents in this course
Academic year: 2020/2021
Listed bookCollins Spanish Dictionary
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Coventry University

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A gas is a loose network of weakly attracted atoms or molecules moving in unpredictable directions. Liquids are less dense than gases. The standard temperature and pressure are zero degrees Celsius (0°C) and one at mare (STP). Liquids, on the other hand, are not miscible with gases. To better explain the behaviour of gases, the kinetic molecular theory was developed as a model of a perfect gas.

The ideal gas has some qualities that aren't present in real gases. These properties include:

  • Gas molecules collide in a totally elastic manner.
  • The volume of gas molecules is zero.
  • Gas molecules' average kinetic energy is directly proportional to their temperature.
  • Gas molecules only have forces when they collide.

Ideal gas law: PV = nRT

V – Volume (in litres) n – Number of moles of gas R – Universal or ideal gas constant (0 L·atm·mol−1·K−1 or 8 J·K−1·mol−1) T – Temperature (in Kelvin)

When the pressure (P) and amount of gas (n) are held constant, Charle's Law states that the volume of a gas (V) is directly proportional to the temperature (in Kelvin). V1/T1 = V2/T

Boyle's Law states that when an ideal gas's volume (V) is kept constant at a constant temperature (T), the pressure and volume are inversely related. P1V1 = P2V

Pure gases and gas mixtures can both benefit from the kinetic molecular theory. Each gas in a container behaves as though it is the only one there. The partial pressure of any gas in a mixture is the amount of pressure the gas contributes to the mixture. As a result, the partial pressure of a certain gas is equal to the total pressure of the gaseous mixture multiplied by its mole fraction.

P(B) = XB. P(total) P(B) – partial pressure of gas B XB – mole fraction of gas B P(total) – total gaseous pressure

Dalton's Law states that a gaseous mixture's total pressure equals the sum of the partial pressures of its constituent gases. This law states that each gas behaves as if it were alone in the container, with the partial pressures of the individual gases adding up to equal the overall pressure. P(total) = P1 + P2 + P3...

Effusion is the spread of a gas from a high pressure to a very low pressure through a smaller hole than the average distance between gas molecules. The gas goes into a vacuum through this tiny aperture.

Diffusion is the process of one gas diffusing into another or into an empty space.

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Gases summary

Module: General and Organic Chemistry (AOC106DI)

26 Documents
Students shared 26 documents in this course

University: Coventry University

Was this document helpful?
A gas is a loose network of weakly attracted atoms or molecules moving in unpredictable
directions. Liquids are less dense than gases.
The standard temperature and pressure are zero degrees Celsius (0°C) and one at mare
(STP).
Liquids, on the other hand, are not miscible with gases.
To better explain the behaviour of gases, the kinetic molecular theory was developed as a
model of a perfect gas.
The ideal gas has some qualities that aren't present in real gases. These properties include:
- Gas molecules collide in a totally elastic manner.
- The volume of gas molecules is zero.
- Gas molecules' average kinetic energy is directly proportional to their temperature.
- Gas molecules only have forces when they collide.
Ideal gas law:
PV = nRT
V – Volume (in litres)
n – Number of moles of gas
R – Universal or ideal gas constant (0.08206 L·atm·mol−1·K−1 or 8.314 J·K−1·mol−1)
T – Temperature (in Kelvin)
When the pressure (P) and amount of gas (n) are held constant, Charle's Law states that the
volume of a gas (V) is directly proportional to the temperature (in Kelvin).
V1/T1 = V2/T2
Boyle's Law states that when an ideal gas's volume (V) is kept constant at a constant
temperature (T), the pressure and volume are inversely related.
P1V1 = P2V2
Pure gases and gas mixtures can both benefit from the kinetic molecular theory. Each gas in
a container behaves as though it is the only one there. The partial pressure of any gas in a
mixture is the amount of pressure the gas contributes to the mixture.
As a result, the partial pressure of a certain gas is equal to the total pressure of the gaseous
mixture multiplied by its mole fraction.
P(B) = XB . P(total)
P(B) – partial pressure of gas B
XB – mole fraction of gas B
P(total) – total gaseous pressure
Dalton's Law states that a gaseous mixture's total pressure equals the sum of the partial
pressures of its constituent gases. This law states that each gas behaves as if it were alone in
the container, with the partial pressures of the individual gases adding up to equal the
overall pressure.
P(total) = P1 + P2 + P3...

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