39. Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. 2 Ag+ (aq) + Pb (s) → 2 Ag (s) + Pb²+ (aq) b. 2 C1O₂ (g) +2 I (aq) → 2 ClO₂¯¯ (aq) + I₂ (s) c. O₂ (g) + 4 H+ (aq) + 2 Zn (s) → 2 H₂O (1) + 2 Zn²+ (aq) 2+

39. Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the half-reaction that occurs at each electrode and the species present in each solution. Also indicate the direction of electron flow. a. 2 Ag+ (aq) + Pb (s) → 2 Ag (s) + Pb²+ (aq) b. 2 C1O₂ (g) +2 I (aq) → 2 ClO₂¯¯ (aq) + I₂ (s) c. O₂ (g) + 4 H+ (aq) + 2 Zn (s) → 2 H₂O (1) + 2 Zn²+ (aq) 2+

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. In an electrochemical cell oxidation and reduction reactions occurs simultaneously, and it is these same reactions which generates electrical energy and powers the cell. a) Clearly identify the difference between an Oxidation and a Reduction reaction. b) Given the overall equation for the cell reaction: 2Cu*(aq) + I2 (aq) → 2Cu²*(aq) + 2I(aq) i. Identify the species which are the oxidizing agent and the reducing agent. Explain your answers. ii. Write the two half equations. iii. Draw the cell diagram iv. Calculate the standard cell e.m.f. v. Suggest whether the cell reaction is feasible. Explain your answer.
Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left half-cell contains 0.115 M Cu(NO₃)₂ (aq). Express your answer to three significant figures.
An unknown metal, X, has been deposited on the cathode of an electrolytic cell using an electric current of 3.30 Amps for a period of 25.0 mins: 2X2+ + 2 e– → X The mass of X collected at the cathode was 1.51 g. Identify the unknown metal, X.
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When an aqueous NaCl solution is electrolyzed, how many coulombs of electric charge need to be transferred at the anode to release 0.130 molmol of Cl2Cl2 gas? 2Cl−(aq)→Cl2(g)+2e−2Cl−(aq)→Cl2(g)+2e−
For each of the reactions, label the half-reaction that is the anode and the reaction that is the cathode in a Galvanic CellI. 1. Cu(s) + 2 Ag*(aq) → Cu²+(aq) + 2 Ag(s) → Zn2+(aq) + H2(g) 2. Zn(s) + 2H*(aq) → Cu(s) → Cu2+(aq) + 2e Choose... + Ag*(aq) + 1e → Ag(s) Choose... + Zn(s) Zn(s) → Zn2+(aq) + 2e Choose... + 2H*(aq) + 2e → H2(g) Choose... + Don Choose... anode cathode
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu?* (aq)+Zn (s) → Cu (s) +Zn²* (aq) Suppose the cell is prepared with 3.40 M Cu´" in one half-cell and 5.47 M Zn2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10
What is the shorthand notation that represents the following galvanic cell reaction? 2 Fe2+ (aq) + Cl2(g) → 2 Fe3+(aq) + 2 Cl-(aq)
1. Mercuric oxide dry-cell batteries are often used where a high-energy density is required, such as in watches and cameras. The two half-cell reactions that occur in the battery are HgO(s)+H2O(l)+2e−→Hg(l)+2OH−(aq) Zn(s)+2OH−(aq)→ZnO(s)+H2O(l)+2e− (a) Write the overall cell reaction. (b) The value of E∘redfor the cathode reaction is +0.098V . The overall cell potential is +1.35V . Assuming that both half-cells operate under standard conditions, what is the standard reduction potential for the anode reaction?
4 A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MSO and the right half cell with a 75.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left right x10 X Ś
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Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --