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The Ideal Gas Law

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Review Recall the equation of the constant (k) for each law: Boyles Lawk B = PV Gay-Lussacs Lawk G = P/T Charless Lawk C = V/T Avogadros Lawk A = V/n

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Review Recall the equation of the constant (k) for each law: Boyles Lawk B = PV Gay-Lussacs Lawk G = P/T Charless Lawk C = V/T Avogadros Lawk A = V/n Combine the four constants …

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A New Constant Emerges Recall the equation of the constant (k) for each law: Boyles Lawk B = PV Gay-Lussacs Lawk G = P/T Charless Lawk C = V/T Avogadros Lawk A = V/n PV nT

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The Ideal Gas Constant The Ideal Gas Constant has the symbol R R = PV nT

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The Ideal Gas Equation The Ideal Gas Constant has the symbol R R = Rearranging this gives the Ideal Gas Law: PV = nRT PV nT

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The Ideal Gas Equation The Ideal Gas Constant has the symbol R R = Rearranging this gives the Ideal Gas Law: PV = nRT PV nT pressure volume moles constant temperature

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The Ideal Gas Equation The Ideal Gas Constant has the symbol R R = Rearranging this gives the Ideal Gas Law: PV = nRT R = 8.314kPa L mol K PV nT

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The Ideal Gas Equation The Ideal Gas Constant has the symbol R R = Rearranging this gives the Ideal Gas Law: PV = nRT R = 8.314kPa L mol K PV nT NOTE: When using this value for R, Pressure must be in kPa, Volume must be in L, and Temperature must be in Kelvin.

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Example 1) Calculate the pressure of mol of He gas at 16.0°C occupying 3.25 L. On board

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Example 2) When 2.50 g of ethanol, C 2 H 6 O, is vaporized, the vapour is found to have a pressure of kPa. The volume of the container is 1.68 L and the temperature is 100°C. What is the molar mass of the ethanol? Hint – Molar mass is the mass in gs of 1 mol of a substance.

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What is an Ideal gas? They dont exist!!!

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What is an Ideal gas? They dont exist!!! An ideal gas is a model for gas behavior that follows the Kinetic Molecular Theory - gas particles are in constant movement - collisions btwn particles and with the container are elastic - there are no attractive or repulsive forces btwn the particles of a gas - do not condense into liquids when cooled

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The Bottom Line At ordinary conditions, most gases behave ideally and obey the gas laws

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