state Avogadro's and Elton law of partial pressure and also drive Dalton's law from kinetic theory of gases
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A) Avogadro's law states that, "equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.
For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.
B)Dalton's law of partial pressure:
In chemistry and physics, Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
This empirical law was observed by John Dalton in 1801 and published in 1802 and is related to the ideal gas laws.
C) Dalton's law of kinetic theory of gases:
According to the kinetic theory of gases ,the attractive forces between the molecules of the same or different gases are very weak under ordinary conditions of temperature and pressure. Therefore the molecules of a gaseous mixture move completely independent of one another. As a result ,each molecule of the gaseous mixture would strike the unit area of the walls of the container the same number of times per second as if no other molecules were present.
Therefore the pressure due to a particular gas is not changed by the presence of other gases in the container. The total pressure exerted by a gaseous mixture must be kept equal to the sum of partial pressure of each gas when present alone in that space. Hence kinetic theory explains Dalton’s law of partial pressure.
Deduction from Kinetic Gas Equation
PV = 1/3 (mnc2)
P= mnc2 / 3V
If only the first gas is enclosed in the vessel of volume V, the pressure exerted would be,
P1 = m1n1c12 / 3V
If second gas is enclosed in the same vessel ,then the pressure exerted would be
P2 = m1n2 c22 /3V
P= m1n1c12 / 3V + m1n2 c22 /3V + ………
P =P1 + P2
Hope it helped.
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For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.
B)Dalton's law of partial pressure:
In chemistry and physics, Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
This empirical law was observed by John Dalton in 1801 and published in 1802 and is related to the ideal gas laws.
C) Dalton's law of kinetic theory of gases:
According to the kinetic theory of gases ,the attractive forces between the molecules of the same or different gases are very weak under ordinary conditions of temperature and pressure. Therefore the molecules of a gaseous mixture move completely independent of one another. As a result ,each molecule of the gaseous mixture would strike the unit area of the walls of the container the same number of times per second as if no other molecules were present.
Therefore the pressure due to a particular gas is not changed by the presence of other gases in the container. The total pressure exerted by a gaseous mixture must be kept equal to the sum of partial pressure of each gas when present alone in that space. Hence kinetic theory explains Dalton’s law of partial pressure.
Deduction from Kinetic Gas Equation
PV = 1/3 (mnc2)
P= mnc2 / 3V
If only the first gas is enclosed in the vessel of volume V, the pressure exerted would be,
P1 = m1n1c12 / 3V
If second gas is enclosed in the same vessel ,then the pressure exerted would be
P2 = m1n2 c22 /3V
P= m1n1c12 / 3V + m1n2 c22 /3V + ………
P =P1 + P2
Hope it helped.
Mark as brainliest.
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