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GASES LAWS - Coggle Diagram
GASES LAWS
GAS LAWS
BOYLE-MARIOTTE'S LAW
This law links pressure and volume, and states that: "The pressure (P) of a gas in a closed container is inversely proportional to the volume (V) of the container, when temperature (T) remains constant."
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CHARLES´ LAW
"The Volume (V of a gas is directly related to the Kelvin temperature (1) when there is no change in gas pressure."
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To study the effect of the temperature change on the volume of a gas, the pressure or quantity of the gas should not change. If the temperature of a gas sample is increased, the kinetic energy will increase; if the pressure is constant, the volume of the gas should increase.
GAY-LUSSAC'S LAW
To study the effect of the temperature change on the pressure of a gas, the volume and number of moles should not be changed. As the temperature increases, the gas molecules move faster, and therefore the number of impacts against the walls increases; that is, the pressure increases, since the the walls of the container are fixed and its volume cannot change.
the ratio between pressure and temperature always had the same value. Mathematically we can put it this way: "Pressure is directly proportional to temperature"
APPLICATIONS : in pressure cookers in which, when the temperature rises, the gas pressure inside will increase
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AVOGADROS LAW
This law establishes that: "When the amount of a gas is increased at constant pressure and temperature, the volume increases in direct proportion because the greater the number of gas particles, the more space is filled."
APPLICATIONS : can be observed in the process of pulmonary respiration: as we know; the lungs have an elastic consistency; that is, they can expand or contract.
IDEAL GAS LAW
The ideal state of any gas refers to its behavior when its molecules are free to interact with each other or with any other external factor; that is, they move freely, with random displacement.
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DALTONS LAW
"The total pressure of a gas mixture is equal to the sum of the pressures exerted by each of the gases that compose it."
APPLICATIONS: measuring the pressure caused by the mixture of gases that constitute the atmosphere using a barometer, or when using a manometer to measure the pressure of the tires of a car
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PROPERTIES OF GASES
The gaseous state differs markedly from solid and liquid states, as it has no defined shape or volume
Diffusion: The process by which a gas is mixed with another, due solely to the movement of its molecules; however, the different gases in a mixture do not separate at rest.
Compression: Reduction in the volume of a gas, because its molecules close in on each other when certain pressure is applied.
Expansion: Gases expand, completely and uniformly, filling the volume of any container.
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