Boyle's law:
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At a fixed temperature, the volume of the given mass of gas is inversely proportional to its pressure.
P ∝ 1/V or PV = constant or P1V1 = P2 V2. This law is perfectly ruled at high temperature and low pressure of a gas.
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Charle's law
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At fixed pressure the volume of a given mass of gas is directly proportional to its absolute temperature.
V ∝ T or V/T = Constant => V1/T1=V2/T2 => V1T2 = V2T1 T1Ρ1= T2 Ρ2
At constant pressure the volume of a given man of gas increases by 1/273 of its volume of 0°C for 1°C gain in its temperature.
Vt = Vo[1+ (1/273)t]
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Gay Lussac's law:
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Gay Lussac's law on kelvin scale defines that volume having constant, the pressure of the required mass of a gas is directly Proportional to its kelvin temperature.
P ∝ T . P1/T1=P2T2
It said that the volume remaining fixed, the pressure of a given man of a gas decrease or increases by 1/273.15 of its pressure at 0°C for each 1°C rise or fall in temperature Pt = Po{1+(1*t)/273.15}
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Dalton's law of partial pressure:
The net pressure exerted by the mixture of in passive gases in a vessel is same to the sum of partial pressure due to individual gases P = P1 + P2 +P3 .......
Avogadro's law:
It defines that same volumes of all gases under identical conditions of pressure and temperature, contain the similar number of molecules. If P1 = P2 ,V1 = V2, T1 = T2 then n1 = n2
Graham's law of diffusion:
It defines that the rates of diffusion of two gases are inversely proportional to the square roots of their densities r ∝1/√Ρ; Where r = Rate of diffusion, Ρ = density of gas.
Ideal gas equation:
It is a relation which relates to the pressure, temperature and volume of the given state of an ideal gas.
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PV = RT
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for 1 mole of gas
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PV = nRT
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for n mole of gas
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PV = rT
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for 1 gram of gas
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PV = nrT
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for n gram of gas
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PV = KT
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for 1 molecule of gas
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PV = nKT
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for n molecule of gas
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R = universal gas constant; r = specific gas constant; k = Boltzmann's constant ; P = pressure
V = volume; T = temperature
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