mole-mass and mole-volume relationships. the mole-mass relationship to convert the mass of a...
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Mole-Mass and Mole-Volume Relationships
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The Mole-Mass Relationship
• To convert the mass of a substance to the number of moles of the substance you have to use the molar mass of an element or compound.
• Mass = # of moles x (mass/1mole)
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The Mole-Mass Relationship
• EX: the molar mass of NaCl is 58.5 g/mol, so the mass of 3.00 mol NaCl is calculated:oMass of NaCl = 3 mol x (58.5 g/1 mol)o = 176 g
• When you measure 176 g of NaCl on a balance, you are measuring 3.00 moles of NaCl.
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The Mole-Mass Relationship Practice
• What is the mass of 9.45 mol of aluminum oxide (Al2O3)?– First add up all the masses• Al = 27g x 2 = 54g• O = 16g x 3 = 48g• Al2O3 = 102 g
– Then convert from moles to grams:• 9.45 mol Al2O3 x (102g/1 mol Al2O3) = 963.9g
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The Mole-Mass Relationship Practice
• 16. Find the mass, in grams, of 4.52 x 10-3 mol C20H42.
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The Mole-Mass Relationship Practice
• 17. calculate the mass, in grams, of 2.50 mol of iron(II) hydroxide Fe(OH)2.
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The Mole-Mass Relationship Practice
• You can calculate the number of moles using the same relationship you use to find the mass of moles by inverting the conversion factor.
• Moles = mass x (1mole/mass)
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The Mole-Mass Relationship Practice
• How many moles of iron(III) oxide are contained in 92.2 g of pure Fe2O3?
• Fe2O3 = 159.6 g = 1 mol
• 92.2 g Fe2O3 x (1 mol/159.6 g Fe2O3) = 0.578 mol Fe2O3
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The Mole-Mass Relationship Practice
• 18. Find the number of moles in 3.70 x 10-1 g boron.
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The Mole-Mass Relationship Practice
• 19. Calculate the number of moles in 75.0 g of dinitrogen trioxide (N2O3)
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The Mole-Volume Relationship
• Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.
• Because of variations due to temperature and pressure, the volume of a gas is usually measured at a standard temperature and pressure.
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The Mole-Volume Relationship
• Standard temperature and pressure (STP) means a temperature of 0C and a pressure of 101.3 kPa, or 1 atmosphere (atm).
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The Mole-Volume Relationship
• At STP, 1 mol or 6.02 x 1023 representative particles, of any gas occupies a volume of 22.4 L.
• The quantity, 22.4 L, is called the molar volume of a gas.
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The Mole-Volume Relationship
• The molar volume is used to convert a known number of moles of gas to the volume of the gas at STP.
• Volume of gas = moles of gas x (22.4L/1mol)
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The Mole-Volume Relationship
• Determine the volume, in liters, of 0.60 mol SO2 gas at STP.
• 1 mol SO2 = 22.4 L SO2
• Volume = 0.60 mol SO2 x (22.4L/1mol)
• = 13 L SO2
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The Mole-Volume Relationship - Practice
• 20. What is the volume of these gases at STP?– A. 3.20 x 10-3 mol CO2
– B. 3.70 mol N2
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The Mole-Volume Relationship - Practice
• 21. at STP, what volume do these gases occupy?– A. 1.25 mol He– B. 0.335 mol C2H6
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Calculating Molar Mass from Density
• Different gases have different densities. Density of a gas is measured in grams per liter (g/L) and at a specific temperature.
• Molar mass = (grams/L) x (22.4 L/1 mole)
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Calculating Molar Mass from Density
• The density of a gaseous compound containing carbon and oxygen is found to be 1.964 g/L at STP. What is the molar mass of the compound?
• Molar mass = (1.964 g/L) x (22.4 L/1 mol)• = 44 g/mol
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Calculating Molar Mass from Density - Practice
• 22. a gaseous compound has a density of 3.58 g/L at STP. What is the molar mass of this gas?
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Calculating Molar Mass from Density
• 23. What is the density of krypton gas at STP?
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