A601. Milwaukie HS Chemistry Linman. Period Date / / In each of the following chemicals, determine the oxidation states of each element:
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1 A601 Assigning Oxidation Numbers In each of the following chemicals, determine the oxidation states of each element: Example: sodium nitrate NaNO 3 12) N 2 O ) ammonia 13) H 2 SO 4 3) zinc oxide 14) SO 2 4) water 5) sulfate anion 15) MnO 2 6) calcium hydride 16) KMnO 4 7) carbon dioxide 17) K 2 Cr 2 O 7 8) nitrogen 18) ClO 4-9) sodium sulfate 19) ClO 2-10) aluminum hydroxide 20) NO 3-11) magnesium phosphate
2 In each of the following reactions, determine what was oxidized and what was reduced. 21) Ca + H 2 O CaO + H 2 Element oxidized: from to Reducing Agent: Element reduced: from to Oxidizing Agent: 22) H 2 + O 2 H 2 O Element oxidized: from to Reducing Agent: Element reduced: from to Oxidizing Agent: 23) PbO 2 + HI I 2 + PbI 2 + H 2 O Element oxidized: from to Reducing Agent: Element reduced: from to Oxidizing Agent: 24) Br 2 + S 2 O H 2 O Br - + SO H + Element oxidized: from to Reducing Agent: Element reduced: from to Oxidizing Agent: 25) Al + NaOH + H 2 O NaAl(OH) 4 + H 2 Element oxidized: from to Reducing Agent: Element reduced: from to Oxidizing Agent:
3 A602 Balancing by Assigning Oxidation Numbers Fe + HCl FeCl 3 + H 2 CaCr 2 O 7 + HCl CaCl 2 + CrCl 3 + H 2 O + Cl 2 HNO 3 (aq) + H 3 PO 3 (aq) NO(g) + H 3 PO 4 (aq) + H 2 O(l)
4 CA601 Balancing by Redox
5 A603 Half Reactions 1. Predict the half-reactions for each of the following chemical or solutions: KF(aq) KNO 3 (aq) K 2 SO 4 (aq) KF(s) An acid solution containing KMnO 4 (aq) 2. Balance the following reaction by the oxidation reduction method. NF3(g) + AlCl3(s)-----> N2(g) + Cl2(g) + AlF3(s)
6 L601 EQUIPMENT: power supply plastic Petri dish Carbon electrodes. MATERIALS : Electrolysis Lab phenolphthalein indicator copper (II) sulfate (0.5 M) potassium iodide (0.1 M) sodium sulfate (0.2M) electrolysis apparatus diagram PROCEDURE: 1. Assemble the electrolysis apparatus as in the above diagram. Place a white piece of paper under the petri dish. 2. Pour 2 ml of the first solution into the Petri dish, add three drops of phenolphthalein, stir the solution and plug in the transformer. 3. Record the first solution's name: Record your electrode observations: 4. Unplug the transformer. Repeat the process for the second solution. 5. Record the second solution's name: Record your electrode observations: 6. Unplug the transformer. Repeat the process for the third solution. 7. Record the third solution's name: Record your electrode observations: CALCULATIONS: 1. Determine the half-reactions for the first solution. 2. Determine the half-reactions for the second solution. 3. Determine the half-reactions for the third solution.
7 QUESTIONS: 1. What are the products of the electrolysis of sodium chloride solution? 2. What are the products of the electrolysis of molten sodium chloride. 3. Using your half-reaction sheet, predict the products of the electrolysis ofa calcium sulfate solution. 3. Using your half-reaction sheet, predict the products of the electrolysis ofa copper(ii) chloride solution.
8 L602 EQUIPMENT: d. c. power source balance two copper strips 100-ml beaker ammeter Faraday s Law Lab MATERIALS: copper(ii) nitrate solution PROCEDURE: 1. Select two copper strips and clean each using a small piece of steel wool. Do not touch the freshly cleaned surfaces. Label one as A and the other as B. 2. Dry the copper strips completely, mass each to the nearest 100th of a gram and enter the mass of each in the mass data table. 3. Pour 50 ml of copper(ii) nitrate in your smallest beaker, and assemble the equipment as in figure A. 4. Plug-in the transformer and check the ammeter to see if it is registering a positive reading. If the ammeter is registering a negative reading, thenreverse the electrical connections on the back of the ammeter. 5. Read and record in the amperes data table the ammeter reading at the end of each minute for twenty minutes. 6. After the last reading gently rinse the copper strips in a beaker of tap water, blot each dry using paper towels followed by hot air drying. 7. After the copper strips are thoroughly dry, remass each and record the mass of each in the mass data table. 8. Return the equipment to the equipment table in a neat and orderly manner. 9. RETURN the copper(ii) nitrate solution to the bottle: It is reusable. COPPER STRIP STRIP A STRIP B MASS DATA TABLE BEFORE REACTION AFTER REACTION AMPERES DATA TABLE figure A
9 CALCULATIONS: 1. Write the half-reaction for the anode reaction. 2. Write the half-reaction for the cathode reaction. 3. Calculate the mass of copper transferred using Faraday's law equation. Answer: 4. How well does the calculated mass change compare with the actual mass change? 5. Calculate the experimental error. Answer: 6. Why can the copper(ii) nitrate solution be used year after year? 7. A current of 4.0 amperes was allowed to flow for 1 hour and twenty minutes. If the current deposited tin metal from a solution of tin(iv) nitrate, how much tin was deposited on the cathode? Answer:
10 L603 EQUIPMENT: volt meter small jar one hole stopper to fit jar Battery Lab MATERIALS: Solution One: copper(ii) sulfate (0.5 M) Solution Two: sodium sulfate (0.5M)/ Hydrochloric acid (0.1 M) copper foil magnesium strip steel wool or other cleaning pad figure A PROCEDURE: 1. Clean a strip of copper and a strip of magnesium using steel wool. 2. Obtain a 25cm strip of dialysis tubing, soak it until it is soft and tie a knot in one end. 3. Fill the jar almost full with sodium sulfate solution. 4. Pour enough copper(ii) sulfate solution in the dialysis tubing to make it full, insert the copper strip in the bag and place the prepared bag in the jar. 5. Put the magnesium strip in the jar. 6. Insert the stopper in the jar so that it holds the bag and magnesium strip as in the figure a. 7. Observe the voltage of the cell using the volt meter. volts: 8. Connect your cell to one of the electric motors supplied by your teacher. 9. See if you can operate the 9-volt radio using your cell. CALCULATIONS: 1. Write the whole-cell reaction and predicted voltage for the cell that you have assembled. whole-reaction: 2. How many cells were in the battery used to operate the Radio? 3. Tell which element is being oxidized 4. Tell which element is being reduced. OVER
11 5. To which half-cell did the negative spectator ions travel? 6. To which electrode did the electrons flow? 7. Which electrode lost mass? 8. Draw and label an electrochemical cell. Use the labels anode, cathode, ion bridge, cation, anion, electric current direction, and spectator ion. 9. What are the factors that affect the E. M. F. of an electrochemical cell. 10. What is a half-reaction? 11. For the following cells, find the half-reaction, the whole-reaction, and calculate the voltage potential. A. Al +3 /Al//Hg2 +2 /Hg whole-reaction: B. Mn +2 /Mn//H +1 /H2 whole-reaction: C. Fe +2 /Fe//Cr +3 /Cr whole-reaction:
12 1. If AgBr(s) undergoes electrolysis, how many grams of material will be produced at the cathode by a current of 19.3 amps flowing for 2.33hours? 2. Balance each reaction using the ion-electron method. a) UO I 2 => U IO 3 - (acidic) b) MnO 2 + I - => MnO I 2 (acidic) 3. Predict the half-reactions for each of the following chemical or solutions: CuF(s) KNO 3 (aq)
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