3: Holey Moley Name: HW 1: The Strange Case of Mole Airlines, Flight 1023 Class: Date:

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1 3: Holey Moley Name: HW 1: The Strange Case of Mole Airlines, Flight 1023 Class: Date: Page 1 of 18 Scenario At 6:02 AM, you and your team of medical examiners are called to the scene of a small airplane crash in a remote location. The plane shows evidence of a pre-crash explosion. Six victims are found at the scene, but none are identifiable by witnesses, dental records, or DNA evidence. The flight manifest shows the names and some information about the victims. You must use the available tools and information to identify each victim, as well as who was responsible for the pre-crash explosion. The Plane A section of the plane has been blown apart by an explosion. It appears as if the explosion happened before the crash. Residue from the explosion site shows was identified as TNT. Passenger Manifest The passenger manifest lists the following passengers who boarded the flight at takeoff. Amadeo Oldere - Pilot with a secret heart condition Norm Anderson Business man with international ties Lisa Johnson - Unemployed, depressed, environmental engineer Bill (Cadillac) Jackson - Car salesman, had a cold Bob (Reno) Henderson - Pro athlete just suspended for drug use Jim LeClaire - Baker Possible Compounds Dimatracine (antidepressant). C10H13N Acetaminophen (Tylenol)... C8H9NO2 Nitroglycerin (explosive or heart medication)... C3H5N3O9 Thiobromine (chocolate flavoring).. C7H8N4O2 Vanillin (vanilla flavoring)... C8H8O3 Codeine (prescription pain killer in cough syrup).. C18H21NO3 Trinitrotoluene (TNT, explosive) C7H5N3O6 Curare (poison).. C40H44N4O Strychnine (rat poison). Cocaine (Narcotic drug) C17H21NO4 Aspartame (Artificial sweetener).. Aspirin (over the counter pain killer)... C9H8O4 C21H22N2O2 C14H18N2O5 GO TO BACK!

2 Directions 1. SHOW ALL WORK ON A SEPARATE SHEET OF PAPER NO WORK, NO CREDIT! This is being collected. 2. Use the percent composition (assume 100 g) to determine the empirical formulas of the samples. 3. Match the empirical formula to the list of possible compounds. 4. Identify which substances where found on whom using the passenger manifest. 5. Determine who blew up the plane. Page 2 of 18 The Victims The following table presents the information obtained from laboratory tests of all the victims. Remember that the bodies were not identifiable, so hopefully we can gain some clues as to the passengers identity based on this laboratory data. Victim # Percent Composition of Sample C H O N Sample Location Blood Empirical Formula Substance Name Victim Name Face, hands Tablets in pocket Pocket, blood Clothing Blood, unlabeled pill bottle

3 3: Holey Moley Name: HW 2: Chemical Equations I Class: Date: Page 3 of 18 For each of the following: Write and balance the chemical equation. 1. When dissolved beryllium chloride reacts with dissolved silver nitrate in water, aqueous beryllium nitrate and silver chloride powder are made. 2. Solid sodium is added to water. A violet explosion takes place; aqueous sodium hydroxide and hydrogen gas are produced. GO TO BACK!

4 Page 4 of Ms. L wants to make some grilled chicken. She lights the butane (C4H10) gas burner on the grill, which reacts with oxygen to form carbon dioxide gas, water vapor, and heat. The heat reacts with the chicken to make dinner. 4. When dissolved sodium hydroxide reacts with dissolved sulfuric acid, aqueous sodium sulfate and liquid water are formed. Heat is also given off.

5 3: Holey Moley Name: HW 3: Chemical Equations II Class: Date: Page 5 of 18 For each of the following: Write and balance the chemical equation. Indicate the type of chemical reaction 1. A solution of lead(ii) nitrate is mixed with a solution of sodium iodide. Lead(II) iodide precipitate and aqueous sodium nitrate are formed. 2. Barium hydroxide solution reacts with hydrochloric acid solution to form aqueous barium chloride and water. GO TO BACK!

6 Page 6 of Copper metal is placed in a solution of silver nitrate, forming copper(ii) nitrate solution and solid silver. 4. A solution of aluminum sulfate is mixed with aqueous calcium hydroxide, forming aqueous aluminum hydroxide and a calcium sulfate precipitate.

7 3: Holey Moley Name: HW 4: Chemical Equations III Class: Date: Page 7 of 18 For the following single replacement reactions, indicate if the reaction will occur or not. If it does, balance the equation. If not, write NR. (HINT: Use the activity series in your unit packet.) 1. Fe + AgNO3 Fe(NO3)2 + Ag 2. H2O + Ca Ca(OH)2 + H2 3. Cl2 + NaF NaCl + F2 4. KI + Br2 KBr + I2 For the following double replacement reactions, indicate if the reaction will occur or not. If it does, balance the equation. If not, write NR. (HINT: Use the solubility guidelines in your unit packet. If H2CO3 is a product, it will break down to form a gas.) 5. NaCl(aq) + H2SO4(aq) Na2SO4 + HCl 6. AgNO3(aq) + NaCl(aq) AgCl + NaNO3 7. H2SO4(aq) + Ba(OH)2(aq) H2O + BaSO4 8. CaCO3(aq) + HCl(aq) CaCl2 + H2CO3 GO TO BACK!

8 Page 8 of 18 For the following reactions, write the chemical equation, balance, and then indicate the type of reaction. 9. Hydrogen peroxide is decomposed by an enzyme to form liquid water and oxygen gas. 10. Barium chloride solution reacts with sodium phosphate solution to form barium phosphate and sodium chloride. One of the products is a solid.

9 3: Holey Moley Name: HW 5: Stoichiometry Calculations I Class: Date: Page 9 of 18 Solve each of the following using dimensional analysis. 1. How many liters of carbon dioxide are prepared when 50.0 moles of calcium carbonate are decomposed? CaCO3 CaO + CO2 2. When 0.50 moles of magnesium react with silver nitrate, how many grams of silver are prepared? Mg + 2 AgNO3 Mg(NO3)2 + 2 Ag 3. If 75.0 g of copper react with mercuric nitrate, how many grams of mercury form? Cu + Hg(NO3)2 Cu(NO3)2 + Hg 4. How many grams of magnesium chloride are produced by treating 4.00 g of titanium (III) chloride with magnesium? 2 TiCl3 + 3 Mg 3 MgCl2 + 2 Ti GO TO BACK!

10 Page 10 of In the electrolysis of 144 g of water, how many moles of oxygen are prepared? 2 H2O 2 H2 + O2 6. The Haber process for synthesizing ammonia, NH3, is shown below. 2 H2 + N2 2 NH3 a. How many moles of ammonia gas are produced when grams of nitrogen react with hydrogen? b. How many liters of ammonia gas are produced? c. Determine the percent yield if 625 liters of ammonia gas are produced. d. Determine the percent yield if 432 grams of ammonia gas are produced.

11 3: Holey Moley Name: HW 6: Stoichiometry Calculations II Class: Date: Page 11 of 18 Solve each of the following using dimensional analysis. 1. If ml of 1.50 M HCl react, how many grams of NaCl can be produced? HCl + NaOH NaCl + H2O 2. The reaction in question 1 was carried out, and 19.9 g NaCl was produced. What is the percent yield?

12 3: Holey Moley Name: HW 7: Stoichiometry Calculations III Class: Date: Page 12 of 18 Solve each of the following using dimensional analysis. Ca(OH)2(s) + HCl(aq) CaCl2(aq) + H2O(l) 1. Balance the chemical reaction. 2. What type of reaction is taking place? 3. How many liters of 0.15 M HCl would be required to react completely with 5.00 grams of Ca(OH)2? 4. If I combined 15.0 grams of Ca(OH)2 with 75.0 ml of M HCl, how many grams of CaCl2 would be formed? (HINT: Do two calculations.) 5. What is the limiting reactant from question 4?

13 3: Holey Moley Name: HW 8: Limiting Reactants Class: Date: Page 13 of 18 Solve each of the following using dimensional analysis. 1. Create a list of steps for solving a limiting reactant problem. 2. How many grams of N2 (molar mass: g/mole) can be obtained by reacting 24.5 g of NH3 (molar mass: g/mole) with 30.8 g of O2 (molar mass = g/mole)? 4 NH3 + 3 O2 2 N2 + 6 H2O GO TO BACK!

14 Page 14 of The first step in the manufacturing process of phosphorous is the reaction below: 2 Ca3(PO4)2 + 6 SiO2 6 CaSiO3 + P4O10 The molar mass of Ca3(PO4)2 is g/mole and the molar mass of SiO2 is 60.1 g/mole. If 20.0 g of Ca3(PO4)2 and 20.0 g of SiO2 are reacted, how many grams of P4O10 can be produced?

15 3: Holey Moley Name: HW 9: Review for Unit Test Class: Date: Page 15 of Consider the unbalanced equation below. NaOH (aq) + H2SO4 (aq) Na2SO4 (aq) + H2O (l) a. What is the limiting reactant if 20.0 grams of NaOH react with 22.5 grams of H2SO4? b. What is the theoretical yield (in grams) of Na2SO4? c. If the total volume if 0.25 L, what is the molarity of the Na2SO4 that was formed? d. Why is it important to know the limiting reactant in a reaction? e. A student performed the reaction above and obtained grams of Na2SO4. What is the percent yield?

16 2. Consider the unbalanced equation below. Page 16 of 18 KOH + CuSO4 K2SO4 + Cu(OH)2 a. How many moles of KOH are needed to produce 12 moles of K2SO4? b. How many moles of CuSO4 are needed to react completely with 4 moles of KOH? 3. A solution is made with grams of NaCl in ml of water. What is the molarity? 4. How many moles of HCl are present in a 10 ml sample of 6M HCl? 5. Consider the reaction below. MgNO3 + X XNO3 + Mg c. What metal could X be such that the reaction occurs? Give two examples. d. What metal could X be such that the reaction does not occur? Give two examples.

17 6. For each of the following, write, balance, and determine the type of reaction. a. Potassium metal and chlorine gas combine to form potassium chloride solid. Page 17 of 18 b. Solid copper and aqueous sulfuric acid react to form aqueous copper (II) sulfate, liquid water, and sulfur dioxide gas. c. Sodium phosphate solution reacts with calcium chloride solution to form sodium chloride solution and calcium phosphate precipitate. 7. For each of the following, predict the products of the reaction, and write out the net ionic equation. a. NaNO3(aq) + Ca(OH)2(aq) b. LiOH(aq) + CuSO4(aq)

18 Page 18 of A group of students was given four bottles of solutions, labeled A, B, C, D. A B C D A NR Solid formed Solid formed NR B Solid formed NR Bubbles NR C Solid formed Bubbles NR Solid formed D NR NR Solid formed NR Use the data to identify each solution. Possibilities are Pb(NO3)2, HCl, Na2CO3, and Ba(NO3)2. Pb(NO3)2 + Pb(NO3)2 Pb(NO3)2 + HCl Pb(NO3)2 + Na2CO3 Pb(NO3)2 + Ba(NO3)2 HCl + Pb(NO3)2 HCl + HCl HCl + Na2CO3 HCl + Ba(NO3)2 Na2CO3 + Pb(NO3)2 Na2CO3 + HCl Na2CO3 + Na2CO3 Na2CO3 + Ba(NO3)2 Ba(NO3)2 + Pb(NO3)2 Ba(NO3)2 + HCl Ba(NO3)2 + Na2CO3 Ba(NO3)2 + Ba(NO3)2