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Answer the following:
a. Will nitrate ions in acidic solution oxidize copper to copper (II) ions?
b. What is the product of the oxidation of copper by iron(II) ions? Copper (I) ions? Copper(II) ions?
5. Which of the following species will be oxidized by 1M HBr?
a. Na
b. Hg
c. Pb
d. Mn2+
6.Consider a voltaic cell at 25oC in which the following reaction takes place
a. Calulate Eo.
b. Write the Nernst equation for the cell.
c. Calculate E under the following conditions:
[NO3-] = 0.750 M
PNO = 0.993 atm
PO2 = 0.515 atm
pH = 2.85
8. A solution containing a metal ion (M2+ (aq)) is electrolyzed by a current of 7.8 A. After 15.5 minutes, 1.19g of the metal is plated out.
a. How many coulombs are supplied by the battery?
b. What is the metal? (Assume 100% efficiency.)
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- 12. Electrochemistry is important in many aspects of daily life. i. Define voltaic cell. ii. Fill in the blanks for the drawing of a voltaic cell that's made with copper/copper (II) nitrate (E° = 0.34 V) and zinc/zinc (II) nitrate (E° = -0.76 V). Briefly explain the role of the salt bridge. iii. Using the equation Eᵒcell = E° cathode E anode, calculate the overall cell potential for the cell in step b. Be sure to show all steps completed to arrive at the answer. h. a. b. C. d. e. 1845 f. g. h. b. C. 9- C. d. harrow_forwardA voltaic (galvanic) cell has a solid lead electrode in a solution of 1.0 mol/L Pb(NO3), and a solid zinc electrode in a solution of 1.0 mol/L Zn(NO3)2. What reactant will be reduced? Zn2+ NO3 Zn Pb2+ Pbarrow_forward4. Consider the voltaic cell: Pb(s) Cla(g) Salt bridge containing NANO;(aq) -1M Pb+ 1M C a. Determine the direction of electron flow and label the anode and the cathode. b. Write a balanced equation for the overall reaction and calculate Ee c. Label each electrode as negative or positive. d. Indicate the direction of anion and cation flow in the salt bridge.arrow_forward
- 2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?arrow_forwardFor each of the following pairs of half-cells: a. Write a balanced chemical equation for each half-reaction and the overall reaction. b. Determine E°cell for the reaction. c. Is the cell spontaneous as written? d. Calculate ΔG°rxn for the cell reaction. Anode: Al(s) Al+3(aq) Ered = -0.1238V Cathode: I2(aq) I-1(aq) Ered = +0.5273V Anode: NO3-1(aq) HNO2(aq) Ered = +0.9513V Cathode: Cr+3(aq) Cr(s) Ered = +0.7237V Anode: ClO4-1(aq) Cl2(aq) Ered = +1.2407V Cathode: Cr2O7-2(aq) Cr+3(aq) Ered = +1.2315Varrow_forward11. The following two half-cells are connected to form a full Galvanic cell: Cu"(aq) +2e Au (aq) +e → Cu(s) → Au(s) E° = 0.34 V E 1.69 V a. Calculate E° for the cell. b. Give the cell notation for this system. c. Give the balanced cell reaction. d. Calculate AG for the reaction e. Calculate Keg for the reaction. £. Calculate the cell potential if the activity of Cu is 0.0100 and the activity of Au" is 1.340.arrow_forward
- For a voltaic cell based on the reaction below, what reaction happens at the cathode?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) a. Zn(s)→Zn2+(aq)+2e- b. 2H+(aq)+2e-→H2(g) c. Zn2+(aq)+2e-→Zn(s) c. H2(g)→2H+(aq)+2e-arrow_forward#26arrow_forwardA charger that supplies a current of 120. mA of current is used to recharge a NiCd battery. How much time, in h, does it take to convert 1.55g of Cd(OH)2 back into Cd so the battery can be used again? O4.73 O 1.25 O 2.29 3.94 O0.732arrow_forward
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