5. What effect, if any, would varying the concentration of both the aqueous species have on thecell potentials? What about varying the size of the electrodes? 4.NameEXPERIMENT 12ELECTROCHEMISTRY: GALVANIC CELLSElectrodesUse the table of standard reduction potentials from your textbook to complete the following table.The zinc-copper Daniell cell is given as an example.CuCuZnZnZnCuZnMgCuMgConc. ofEach Cation1.0 M Zn²+0.5 M Cu²+1.0 M Zn²+0.1 M Cu²+Date1.0 M Zn²+Zn²+ + 2e-Zn(ag)Half-ReactionsA. Determine the E for the Standard Zn-Cu Galvanic CellZn²+(aq)1.0 M Cu²+Cu²++2e-CuCathodeB. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations1.0 M Zn²+Anode+ 2e → ZnInstructorCu²+2e-CuZn²+ + 2e → Zn(aq)Report SheetCathode orAnode?AnodeEE(table) (calcd)-0.76 V+0.34 V-0.76VCathode 0.34 vanode 0.76vCathode 0.34 vCu²+ + 2e - CulC. Determine the E for Zn-Mg and Cu-Mg Galvanic CellsZn(aq) +2e Zn (s) cathode -0.761.0 M Mg²+Mga+2e Mg(s) anode -2.38+1.10 V1.10 V1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v2+ +2e1.0 M Mg²+ MMg(s) anode -2.38v"You must use the Nernst equation to calculate this Ecell voltage. (See Equation 8.)1.62 v1.10 0.98 vEº(measured)2.72v+1.06 x1.04 v1.54 v1.99 vVELECTROCHEMISTRY: GALVANIC CELLS 141M

On changing the concentration ,changes can be observed in the E° measured values. This can be shown…

Answered: 5. What effect, if any, would varying…

5. What effect, if any, would varying the concentration of both the aqueous species have on the cell potentials? What about varying the size of the electrodes?

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...

See similar textbooks

Similar questions

Explain the following relationships: Delta G and w, cell potential and w, cell potential and Delta G, cell potential and Q. Using these relationships, explain how you could make a cell in which both electrodes are the same metal and both solutions contain the same compound, but at different concentrations. How could this cell run spontaneously?
75. Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should include a working electrode, a reference electrode, and a counter electrode. (B) The pH meter is unable to determine the pH of 0.1 M NaOH. (C) Silver chloride-coated silver wire is commonly used as a reference electrode in the pH meter. (D) The glass membrane must be hydrated. (E) The difference in potential between the inner and outer layers is the boundary potential.
Will the potential of the galvanic cell change if we add the same amount of water to the electrolyte solutions that make up the galvanic cell?
The silver zinc battery is used in hearing aids. Explain the fundamental redox reactions that occur in this battery and calculate the theoretical cell potential for this system.
(iv) raised from 25 °C to 100 °C? Which of the following would result for any cell if the temperature was A. The cell potential would not change at all B. The cell potential would increase slightly C. The cell potential would decrease slightly D. It is impossible to determine. E. It would depend on the nature of the electrodes used.
Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…
1
Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness.
the Faraday constant. Suppose that after the electroplating was complete, you wiped the cathode copper strip very harshly with a tissue wipe (wiping off some of the electroplated copper off the strip) How would this specifically affect your calculated value of the Faraday constant?
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGO. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell n A U calculated quantities (Check the box next to any that are wrong.) AGⓇ -117. kJ/mol - 129. kJ/mol 112. kJ/mol K 3.18 × 10 2.51 X 10 4.18 × 10 21 - 23 19 0 E 1.21 V - 1.34 V 1.16 V
Which statement about electrolytic cells is false? Electrolytic cells convert electrical energy into chemical energy. O The redox reaction is non-spontaneous. The anode and cathode are placed in the same container with the aqueous electrolyte. O The anode is negative and the cathode is positive. O The external battery supplies the electrons.