Name: ___________________________ Score: __________ Section: ___________ Date: ___________ I. Enumeration: 1-5 Subbranches of Chem 6-7. properties of matter 1. 6. 2. 7. 3. 8-10 types of heterogeneous mixture 4. 8. 5. 9. II. Identify how many significant digits are present ___1. 0.5789 ___6. 27.00 ___2. 1000000.01 ___7. 04.68 x 1023 ___3. 1.805 x 108 ___8. 562 ___4. 100023.00 ___9. 29.00 ___5. 50.00 ___10. 72.00001 III. Conversion 1. 39.2 tons -> tg 2. 45.74 inch -> miles 3. 98213 lbs -> ng 10. IV. Specific heat 1.A block of aluminum weighing 140 g is cooled from 98.4°C to 62.2°C with the release of 1080 joulesof heat. From this data, calculate the specific heat of aluminum. 2.100.0mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J/g°C, calculate the amount of heat energy needed to cause this rise in temperature.(Note: 1 ml of water = 1 gram) 3.Object A specific heat is 2.45 J/g∙°C and object B specific heat is 0.82 J/g∙°C. Which object will heat up faster if they have the same mass and equal amount of heat is applied? Explain why. V. STOICHIOMETRY a. Convert the following number of moles of chemical into its corresponding mass in grams. 1. 0.436 moles of ammonium chloride 2. 2.360 moles of lead (II) oxide 3. 0.031 moles of aluminium iodide 4. 1.077 moles of magnesium phosphate 5. 0.50 moles of calcium nitrate b. Convert the following masses into their corresponding number of moles. 6. 23.5 g of sodium chloride 7. 0.778 g of sodium cyanide 8. 0.250 g of water 9. 169.45 g of calcium acetate 10. 79.9 g of potassium permanganate 11. Using the following equation: Fe2 O3+ H2 -------------> Fe + H2O Calculate how many grams of iron can be made from 16.5 grams of Fe2O3 by the following equation. 12. Using the following equation: I2 + KIO2 + HCl ---------> ICl + KCl + H2O Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction. 13. Using the following equation: KNO2 + KMnO4 + H2SO4 ------> KNO3 + MnSO4 + K2SO4 + H2O How many moles and how many grams of KMnO4 are needed to carry out this reaction on 11.4 grams of KNO2? VI. Percent yield 1. If, in the reaction below 32 grams of C2H6 produces 44 grams of CO2, what is the % yield? 2C2H6 + 7O2 -> 4CO2 + 6H2O 2. If, in the reaction below, 80 grams of Cl2 produces 38 grams of CCl4 what is the % yield CS2 + 3Cl2 -> CCl4 + S2Cl2 3. If, in the reaction below, 49 grams of Fe3O4 produces a 78.25 % yield of Fe. How many grams are produced? Fe3O4 + 4H2 -> 3Fe + 4H2O VII. Limiting Reactants 1.BALANCE the equation first. FeCl3 + O2 -> Fe2O3 + Cl a. How many moles of chlorine gas can be produced if 4 moles of FeCl3 react with 4 moles of O2? b. What is the limiting reactant? c. What is the excess reactant? 2.Use the following BALANCED equation. 2 C2H6 + 7 O2 -> 4 CO2 + 6 H2O a.If 15 g of C2H6 react with 45 g of O2, how many grams of water will be produced? b. What is the limiting reactant? c. What is the excess reactant?