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Mole

Mole. Stoichiometry. The study of quantitative relationships between the amounts of reactants used and products formed by a chemical reactions; it is based on the law of conservation of mass. Mole. The SI base unit used to measure the amount of a substance. Avogadro’s Number.

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Mole

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  1. Mole

  2. Stoichiometry The study of quantitative relationships between the amounts of reactants used and products formed by a chemical reactions; it is based on the law of conservation of mass.

  3. Mole The SI base unit used to measure the amount of a substance.

  4. Avogadro’s Number The number of representative particles in a mole, and can be rounded to three significant digits: 6.02 X 1023 molecules/mol

  5. moles/L =M Molarity

  6. Molecule Forms when two or more atoms covalently bond.

  7. To find the number of molecules it takes to equal a certain number of moles. Take the number of moles given and multiply by Avogadro’s number.

  8. How many molecules of Sucrose is in 3.50 moles of Sucrose. 3.50 mol Sucrose X 6.02x1023 molecules/mol =2.11x1024molecules of Sucrose

  9. How many molecules of Sodium Hydroxide is in 4.80 moles of Sodium Hydroxide? 4.80 mol Sodium Hydroxide X 6.02x1023molecules/mol =2.89x1024 molecules of Sodium Hydroxide

  10. To find the number of moles it takes to equal a certain number of molecules. Take the number of molecules given and divide by Avogadro’s number.

  11. How many moles of Sucrose is in 3.54x1024 moleculesof Sucrose. 3.54x1024 molecules of Sucrose ÷ 6.02x1023 molecules/mol =5.88 moles of Sucrose

  12. How many moles of Sodium Hydroxide is in 5.63x1024 moleculesof Sodium Hydroxide. 5.63x1024 molecules NaOH ÷ 6.02x1023 molecules/mol =9.35 moles of NaOH

  13. Molar Mass The mass in grams of one mole of any pure substance. g/mol

  14. To find the number of grams of substance. Take the number of moles given and multiply by the substance’s molar mass.

  15. Find the mass of 3.2 moles of Butane needed to complete the reaction. 3.2 mol of Butane X 58.14 g/mol =186.05 g of Butane

  16. Find the mass of 4.5 moles of Pentanol needed to complete the reaction. 4.5 mol Pentanol X 86.15 g/mol =387.68 g of Pentanol

  17. To find the number of moles of substance. Take the number of grams given and divide by the substance’s molar mass.

  18. Find the moles of 23 g of water needed to complete the reaction. 23 g water ÷ 18.02 g/mol =1.28 mol of water

  19. Find the moles of 112 g of Hydrochloric Acid needed to complete the reaction. 112 g of Hydrochloric Acid ÷ 36.46 g/mol =3.07 mol of Hydrochloric Acid

  20. To find the number of moles of an element in a compound, multiply the moles of the compound with the ratio of number of elements to 1 mol of compound.

  21. How many moles of Fluorine is found in 5.50 moles of Freon (CCl2F2). 5.50 mol CCl2F2X 2 mol F atoms/1 mol CCl2F2 = 11.0 mol F atoms

  22. How many moles of Oxygen is found in 4.75 moles of Glucose (C6H12O6). 4.75 mol C6H12O6 X 6 mol O atoms/1 mol C6H12O6 = 28.5 mol O atoms

  23. To find the moles of a compound, take the mass of the compound and divide by the molar mass of the compound.

  24. How many moles are there of 47g of water? 47g of water ÷ 18.02 g/mol of water = 2.61 mol of water

  25. How many moles are there of 21g of Benzene? 21g of Benzene ÷ 78.12 g/mol of Benzene = 0.27 mol of Benzene

  26. Mole Ratio In a balanced equation, the ration between the numbers of moles of any two substances.

  27. To find mole ratio, put moles of one substance over the moles of another substance in chemical equation. 2KClO3 → 2KCl + 3O2 2mol KClO3/2mol KCl 2 mol KClO3/3mol O2

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