10.5 NOTES Avogadro Molar Volumes

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Presentation transcript:

10.5 NOTES Avogadro Molar Volumes

B. Avogadro’s Principle - equal volumes of gases @ same temp and pressure contain equal #’s of particles - 1 mole contains 6.022 x 1023 particles - equal #’s of particles have same volume, but not necessarily same mass  1 mol of H2 @ STP = 22.4 L = 6.02 x 1023 molecules = 2.02 g 1 mole of N2 @ STP = 22.4 L = 6.02 x 1023 molecules = 28.0 g Molar volume = 22.4 L at STP One mole of a gas occupies 22.4L at STP (0.00°C and 1.00 atm)

Determine the volume of 0.881 mol of a gas at STP. V = 0.881 mol x 22.4 L 1 mol = 19.7 L

Find V, given 2.00kg CH4 at STP. 1 kg 16.0g 1 mol = 2.80 x 103 L kg x 1000g x 1 mol x 22.4 L 1 kg 16.0g 1 mol = 2.80 x 103 L

How many moles are in a 2.50 L? Moles = 2.50 L x 1 mol 22.4 L = 0.112 mol

What is the density of hydrogen sulfide at STP? H2S = 34.1 g x 1 mol 1 mol 22.4 L = 1.52 g/L

A sample of gas has a mass of 3 A sample of gas has a mass of 3.89 grams and occupies a volume of 450 mL at STP. What is the molar mass of the gas? MM = 3.89 g x 22.4 L .450 L 1 mol = 194 g/mol