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Unit-3-Notes 1- Gases-1

# Unit-3-Notes 1- Gases-1 - Keywords Boyles law Charles law...

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Keywords Boyles law Charles law Gay-Lussac’s law Avogadro’s law Ideal gas law Gas constant Dalton’s law of partial pressure Mole fraction Kinetic molecular theory Diffusion Effusion Absolute temperature Molecular velocity

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1. Compressibility (P, V, T) a. Boyles Law P α 1/V at constant T and n b. Charles Law V α T at constant P and n Gay-Lussac V T° C = V 0° C ( 1 + T° C/273)
Boyles Law P α 1/V at constant T and n

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2. Relationship between V and n a. Gay-Lussac’s Law of Combining Volumes b. Avogadro’s hypothesis V α n at constant T and P Equal volume of gases under the same condition of temperature and pressure contains the same number of molecules

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3. Equation of State Boyle PV = constant 1 Charles V = T x constant 2 Avogadro V = n x constant 3 PV = T x n x constant PV = nRT IDEAL GAS LAW
Gas Constant R = PV/ nT n T V P 1 273.15 K 22.414 L 1 atm 760 torr STP 101.3 kP R = 0.08205 L atm / K mol = 62.36 L torr / K mol = 8.314 J / K mol = 1.987 cal / K mol (1 cal = 4.184 J)

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One mole of an ideal gas occupies a volume of 22.414 L at STP. This is called molar volume. From this we can calculate the ……………………………………………………………………………………… ……………………………………………………………………………………… ……………………………. For eg. How many moles are there in 10 L of a gas at STP It is ……………………………………………………. How many molecules are there in 10 L …………………………………………………………………… [ …………………………………………………………………………………… ……………………..]
Assuming ideal behaviour predict which one will contain more number of molecules 2.2 L H 2 or 2.2 L CO 2 Which one will have a greater volume at STP?

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Unit-3-Notes 1- Gases-1 - Keywords Boyles law Charles law...

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