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9 Week Spring Review

9 Week Spring Review. Chemistry. Zn + 2HCl → ZnCl 2 + H 2. Mixed Example. #2. If 3.4 mol of HCl are used in this reaction, how many grams of zinc (II) chloride are produced?. C 3 H 8 + 5O 2 → 3CO 2 + 4H 2 O. Mixed Example. #1.

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9 Week Spring Review

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  1. 9 Week Spring Review Chemistry

  2. Zn + 2HCl → ZnCl2 + H2 Mixed Example #2 If 3.4 mol of HCl are used in this reaction, how many grams of zinc (II) chloride are produced?

  3. C3H8 + 5O2→ 3CO2 + 4H2O Mixed Example #1 If 3.2 mol of oxygen are consumed in the above reaction, how many grams of water are produced?

  4. Limiting Reactants How many moles of NH3 can be produced from the reaction of 28g of nitrogen and 25g of hydrogen? Using the following equation identify the limiting reagent. N2 + 3H2 2NH3

  5. Limiting Reactants Mg + 2HCl → MgCl2 + H2 How many grams of magnesium chloride are produced from the reaction of 2.08 mol of Mg and 2.08 mol of HCl?

  6. Limiting Reactants 2KBr + Cl2→ 2KCl + Br2 How many moles of KCl are produced from the reaction of 20.3g of KBr and 20.3g of chlorine?

  7. Percent Yield Percent yield- the ratio of the actual yield to the theoretical yield Actual yield- the amount of product formed when a reaction is carried out in the laboratory Theoretical yield- the calculated amount of product formed during a reaction

  8. Percent Yield measured in lab calculated on paper

  9. Percent Yield When 45.8 g of K2CO3 react with excess HCl, 46.3 g of KCl are formed. Calculate the theoretical and % yields of KCl. K2CO3 + 2HCl  2KCl + H2O + CO2 Unknown = g KCl Known = 45.8 g K2CO3 Actual: 46.3 g

  10. Output side 1. Which of the following compounds dissolved the highest at 20°C? 2. The lowest at 20°C? 3. Overall which compound dissolved the fastest? 4. Name a compound in the graph that is a gas? How do you know it’s a gas?

  11. A. Molarity • Calculate the number of moles in 1 L of the solution Molarity (M) = moles of solute liters of solution Example 1 Calculate the molarity when 2 mol of glucose is dissolved in 5 L of solution, divide the number of moles by the volume in liters. 2 mol glucose 5 L solution = 0.4 mol/L = 0.4 M

  12. Finding the pH of Solutions Self- ionization of water – the simple dissociation of water H2O H+ + OH- Concentration of ea. ion in pure water: [H+] = 1.0 x 10-7M + [OH-] = 1.0 x 10-7M Ion-product constant for water (Kw),Where Kw = 1.0 x 10-14 Kw = [H+] [OH-] Acid [H+] > [OH-] Base [H+] < [OH-] Neutral [H+] = [OH-]

  13. Example If the [H+]in a solution is 1.0 x 10-5M, is the solution acidic, basic or neutral? 1.0 x 10-5 M What is the concentration of the [OH-]? Use the ion-product constant for water (Kw): Kw = [H+] [OH-] 1.0 x 10-14 = [1.0 x 10-5] [OH-] 1.0 x 10-14 = [OH-] 1.0 x 10-5 1.0 x 10-(14-5) pH 5 = acidic 1.0 x 10-9 OH-

  14. pH Scale pH paper and digital probes give a more accurate reading of the pH of a substance

  15. Formulas to Use Mole - Mole Known mol of unknown mol of known Mol Ratio – from equation Mass - Mass mol of unknown Known g 1 mol known molar mass unknown mol of known 1 mol unknown molar mass known OR OR Other 6.02 × 1023 particles mol of unknown Known L 1 mol known 22.4 L unknown OR mol of known 1 mol unknown particles 22.4 L known 6.02 × 1023 particles

  16. Your clothing labels have Percent Composition.

  17. Percent Composition molar mass of compound • The percent by mass of each element in a compound • Information needed: • Formula of the compound • Gram atomic mass of its elements % mass = grams ofelement in 1 mol compound× 100

  18. Calculating % Composition grams of compound grams of compound 44g • Calculate the % composition of C3H8. • % C = mass of C × 100 = 36g X 100% = 0.818181 = 81.8% 44g • % H = mass of H × 100 = 8g × 100% = 0.181818 = 18%

  19. Neutralization • Chemical reaction between an acid and a base. • Products are a salt (ionic compound) and water.

  20. Neutralization ACID + BASE  SALT + WATER HCl + NaOH  NaCl + H2O strong strong neutral HC2H3O2 + NaOH NaC2H3O2 + H2O weak strong basic

  21. Empiracal Formula • Empirical Formula- The lowest shole-number ratio of the elements in a compound • Concentration of ions- High concentration for a base –OH High concentration for an acid H+ • Gram Formula Mass- Add all the atoms present for the total mass

  22. The MoleRoad Map Molecule Atoms (ions) Formula unit

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