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Hydrates and Molar Volume of Gases

Hydrates and Molar Volume of Gases. Section 11.5. What is a Hydrate?. A compound that has a specific number of water molecules bound to its atoms Examples: Sponges Opals CaCl 2 – Desiccant. Naming Hydrates. Desiccators.

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Hydrates and Molar Volume of Gases

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  1. Hydrates and Molar Volume of Gases Section 11.5

  2. What is a Hydrate? A compound that has a specific number of water molecules bound to its atoms Examples: Sponges Opals CaCl2 – Desiccant

  3. Naming Hydrates

  4. Desiccators • * The anhydrous form of a hydrate used to absorb water. • *Anhydrous compounds can be packaged with materials that need to be kept moisture free • Can you think of any examples?

  5. Steps to Determining Anhydrous Formulas • Determine the number of moles of the compound by dividing the mass by the molar mass. • Determine the number of moles of water by dividing the mass by the molar mass. • 3. Divide by the smallest number of moles. • Determine the ratio. • Please Copy the Steps Down!!!!

  6. Hydrates Practice Problems What is the mole ratio of the hydrate CuSO4 . ____ H2O, if the anhydrous mass of the CuSO4 is 25.42g and the mass of the water is 14.3g? What is the mole ratio of the hydrate Na2CO3 . _____ H2O, if the original mass of the hydrated Na2CO3 was 43.69 g and the mass of the anhydrous Na2CO3 is 16.19 g? Determine the empirical formula for a compound found to contain 25.38 g of Mg and 74.62 g of Cl by mass. Determine the empirical formula for a compound that contains 32.88 % Carbon, 1.37 % Hydrogen, and 65.75 % Oxygen by mass.

  7. Molar Volume of Gases Avogadro’s Principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. The Molar Volume for a gas is the volume that one mole occupies at 0°C and 1.00 Atmospheres (atm) of pressure. These conditions are known as STP (Standard Temperature and Pressure). Avogadro showed experimentally that one mole of any gas will occupy a volume of 22.4 L at STP. The following conversion factor can be used to find the number of moles, the mass, and even the number of particles in a a gas sample. 22.4 L 1 mol

  8. Molar Volume of Gases Practice • How many moles does 44.8 L of Hydrogen gas at STP represent? • A sample of oxygen gas occupies 6.2 L at STP.   How many moles does that represent? • 3. How many liters will 23.50 g of nitrogen occupy at STP? • How many liters will 100 grams of oxygen occupy @ STP? • 5. How many grams of oxygen would be required to occupy 11.2 L at STP?

  9. Volume of Gases Practice 6. A sample of chlorine gas occupies 72.3 L @ STP. How many grams of chlorine gas are present? 7. How many moles of hydrogen gas are present in 162.4 liters @ STP? 8. How many grams of lithium gas would be required to fill a 50 liter container @ STP? 9. A sample of bromine gas occupies 28.3 liters @ STP. How many grams of bromine gas are present? 10. What is the mass of 857 liters of nitrogen gas @ STP?

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