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 10 23 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 6.02x10 23 molecules/mol =2.11x10 24 molecules of Sucrose

9. How many molecules of Sodium Hydroxide is in 4.80 moles of Sodium Hydroxide? 4.80 mol Sodium Hydroxide X 6.02x10 23 molecules/mol =2.89x10 24 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 3.54x10 24 molecules of Sucrose. 3.54x10 24 molecules of Sucrose ÷ 6.02x10 23 molecules/mol =5.88 moles of Sucrose

12. How many moles of Sodium Hydroxide is in 5.63x10 24 molecules of Sodium Hydroxide. 5.63x10 24 molecules NaOH ÷ 6.02x10 23 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 (CCl 2 F 2 ). 5.50 mol CCl 2 F 2 X 2 mol F atoms/1 mol CCl 2 F 2 = 11.0 mol F atoms

22. How many moles of Oxygen is found in 4.75 moles of Glucose (C 6 H 12 O 6 ). 4.75 mol C 6 H 12 O 6 X 6 mol O atoms/1 mol C 6 H 12 O 6 = 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. 2KClO 3 → 2KCl + 3O 2 2mol KClO 3 /2mol KCl 2 mol KClO 3 /3mol O 2