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The Mole

The Mole. Chapter 10. Previous Skills required for this chapter. Writing formulas from names for: Ionic compounds Covalent compounds Acids Balancing equations Predicting Products Minor emphasis, but still needed. Skills to be learned. Determining molar mass Elements Compounds

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The Mole

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  1. The Mole Chapter 10

  2. Previous Skills required for this chapter • Writing formulas from names for: • Ionic compounds • Covalent compounds • Acids • Balancing equations • Predicting Products • Minor emphasis, but still needed

  3. Skills to be learned • Determining molar mass • Elements • Compounds • Determining number of moles within a compound • Molar conversions • Mole to mole; gram to mole; mole to gram; gram to mole; mole to atoms; atoms to mole • Empirical Formula and Molecular formula • Formulas and naming hydrates

  4. The mole, what is it?

  5. Mole • 6.02x1023 atoms • For a given molecule, one mole is a mass (in grams) whose number is equal to the atomic mass of the molecule. • In general, one mole of any substance contains Avogadro's Number of molecules or atoms of that substance. • This relationship was first discovered by Amadeo Avogadro (1776-1858) and he received credit for this after his death.

  6. Molar mass • Unit: g/mol • The amount of mass (in grams) for every one mole of the element or molecule. • For elements:

  7. Molar Mass • For compounds

  8. Conversion factors of molar mass

  9. Empirical and molecular formulas • Percent composition from experimental data

  10. Empirical and molecular formulas • Percent composition from the chemical formula

  11. Problems • What is the percent composition of phosphoric acid? • Which has the larger percent by mass of sulfur: H2SO3 or H2S2O8? • Calcium chloride is sometimes used as a de-icer. Calculate the percent by mass of each element in CaCl2. • Challenge: Sodium sulfate is used in the manufacture of detergents. • Identify each of the component elements of sodium sulfate, and write the compound’s chemical formula. • Identify the compound as ionic or covalent. • Calculate the percent by mass of each element in sodium sulfate.

  12. Empirical Formula • Empirical formula is the formula with the smallest whole-number mole ratio of the elements. • Steps to finding empirical formula. • Given Percent by mass. • Convert to moles. • Determine the smallest value. • Divide all numbers by smallest value. • If whole numbers, they are the subscripts. If they are not, multiply in order to reach a whole number.

  13. Step One: Given Percent by mass • If given percentage, turn % into g. • If given grams, continue on.

  14. Step Two: Convert to moles.

  15. Step Three: Determine the smallest value.

  16. Step Four: Divide by smallest number.

  17. Step Five: Answer?

  18. Problems • Determine the empirical formula for a compound that contains 35.98% aluminum and 64.02% sulfur. • Propane is a hydrocarbon, a compound composed only of carbon and hydrogen. It is 81.82% carbon and 18.18% hydrogen. What is the empirical formula? • Aspirin is the world’s most-often used medication. The chemical analysis of aspirin indicates that the molecule is 60.00% carbon, 4.44% hydrogen, and 35.56% oxygen. Determine the empirical formula for aspirin.

  19. Molecular Formula • Molecular formula specifies the actual number of atoms of each element in one molecule or formula unit of the substance. • Steps to determine Molecular formula • Given Percent by mass. • Convert to moles. • Determine the smallest value. • Divide all numbers by smallest value. • If whole numbers, they are the subscripts. If they are not, multiply in order to reach a whole number. • Determine the molar mass of the EF (answer from previous step) • Divide molar mass of EF by molar mass of MF (given) • Multiply EF by answer in previous step.

  20. Step One: Given Percent by mass • If given percentage, turn % into g. • If given grams, continue on.

  21. Step Two: Convert to moles.

  22. Step Three: Determine the smallest value.

  23. Step Four: Divide by smallest number.

  24. Step Five: Answer?

  25. Step Five: Empirical Formula

  26. Last o’ the steps:

  27. Problems • A compound was found to contain 49.98g of carbon and 10.47g of hydrogen. The molar mass of the compound is 58.12g/mol. Determine the molecular formula. • A colorless liquid composed of 46.68% nitrogen and 53.32% oxygen has a molar mass of 60.01g/mol. What is the molecular formula? • When an oxide of potassium is decomposed, 19.55g of K and 4.00g of O are obtained. What is the empirical formula?

  28. Formulas of Hydrates • Hydrate is a compound that has a specific number of water molecules bound to its atoms. • Naming Hydrates on next slide • Anhydrous – without water

  29. Steps for determining hydrate formulas • Determine given • Determine mass of water lost • Convert masses to moles • Solve for ratio of moles of water to moles of solid • Write formula

  30. Step One • A 20g sample of a hydrate of nickel sulfate (NiSO4) lost 9.63g of water when heated. Determine the hydrate’s formula. • Hydrate is 20g • Water lost 9.63g

  31. Steps continued. . .

  32. Problems • An 11.75g sample of a common hydrate of cobalt(II) chloride is heated. After heating, 0.0712 mol of anhydrous cobalt chloride remains. What is the formula and name of this hydrate?

  33. Uses of hydrates • Hydrates absorb water • Desiccants prevent moisture from intergering with the sensitive electronic circuitry • Some store solar energy • When the Sun’s energy heats the hydrate to a temperature greater than 32 degrees Celsius, the single formula unit of Na2SO4 in the hydrate dissolves in the 10mol of water of hydration. In the process, energy is absorbed by the hydrate. This energy is released when the temperature decreases and the hydrate crystallizes again.

  34. The End

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