80. Consider the concentration cell:Pb(s)Salt bridgecontainingNaNO3(aq)2.5 M Pb2+5.0 × 10 ³M Pb2+a. Label the anode and cathode.Pb(s)b. Indicate the direction of electron flow.c. Indicate what happens to the concentration of Pb2+ in eachhalf-cell.

Anode is where oxidation occurs, and cathode is where reduction occurs. Oxidation is the process of…

Answered: 80. Consider the concentration cell:…

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. What mass of lead is deposited on the cathode during the electrolysis of lead (II) sulphate solution if 3 amps flows for 17 minutes? Electrode equation: Pb²* + 2e* → Pb RAM Pb= 64 1 Faraday= 96 500 C 4. How long will it take to deposit 1.5 g of aluminium on the cathode during the electrolysis of aluminium sulphate solution using a current of 4A? Electrode equation: Al3+ (aq) 3+e→ Fe (s) RAM Al= 27 1 Faraday= 96 500 C 5. What mass of magnesium is deposited on the cathode during the electrolysis of magnesium chloride solution if 17 amps flows for 2 days and 3 minutes? Electrode equation: Mg²+ + 2e → Mg RAM Mg= 24 Quantitative Electrolysis Handout Grade 10 1 Faraday= 96 500 C 6. How long will it take to deposit 17 g of sodium on the cathode during the electrolysis of sodium nitrate solution using a current of 2A? Electrode equation: Na* (aq) +e* → Na (s) RAM Na= 23 1 Faraday= 96 500 C
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?
Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.
23
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which [Cu²+] = 5.9 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown [Cu²+ ]. The measured potential at 25°C is 0.222 V. What is [Cu²+ ] ? (Assume Cu²+ is reduced.) [Cu²+] = M
Zn(s) + 2 H*(aq) → Zn²*(aq) + H2(g) 1. What is the effect on the cell potential of a voltaic cell wi h the above reaction when: The pressure of H2 gas is increased in the cathode. c. Sodium hydroxide is added to the cathode half-cell decreasing the [H"]. а. b. Zinc nitrate is added to the anode d. The surface area of the anode is doubled. half-cell.
11. 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.
4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…

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80. Consider the concentration cell: Pb(s) Salt bridge containing NaNO3(aq) 2.5 M Pb2+ 5.0 × 10 ³M Pb2+ a. Label the anode and cathode. Pb(s) b. Indicate the direction of electron flow. c. Indicate what happens to the concentration of Pb2+ in each half-cell.