Questions 25-28 cover aspects of real-life applications of electrochemistry. This will allow you to see application and relevance of the concepts you have studied in this topic. Question 25: A fuel cell is a(n) voltaic cell half cell concentration cell electrolytic cell galvanic cell Check Reuse <> Embed Question 26: A hydrogen fuel cell produces in its overall redox reaction hydrogen oxygen water Check Reuse <> Embed Question 27: What is the anode material in a dry cell battery? ○ Zn graphite Mn2O3 MnO2 ○ NH4+ Check Reuse <> Embed Question 28: What is the anode material in a nickel-cadmium battery? ○ Cd Ni ○ NiO2 graphite OH- Check Reuse <>Embed H-P H-P H-P H-P

Questions 25-28 cover aspects of real-life applications of electrochemistry. This will allow you to see application and relevance of the concepts you have studied in this topic. Question 25: A fuel cell is a(n) voltaic cell half cell concentration cell electrolytic cell galvanic cell Check Reuse <> Embed Question 26: A hydrogen fuel cell produces in its overall redox reaction hydrogen oxygen water Check Reuse <> Embed Question 27: What is the anode material in a dry cell battery? ○ Zn graphite Mn2O3 MnO2 ○ NH4+ Check Reuse <> Embed Question 28: What is the anode material in a nickel-cadmium battery? ○ Cd Ni ○ NiO2 graphite OH- Check Reuse <>Embed H-P H-P H-P H-P

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.28QAP

See similar textbooks

Similar questions

The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V
Determine the overall reaction and its standard cell potential at 25 C for this reaction. Is the reaction spontaneous at standard conditions? Cu(s)|Cu2+(aq)Au3+(aq)|Au(s)
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
A galvanic cell is constructed in which the overall reactionis Cr2O72(aq)+14H2O+(aq)+6I(aq)2Cr3+(aq)+3I2(s)+21H2O(l) Calculate E for this cell. At pH 0, with [Cr2O72]=1.5M and [I]=0.40M, the cell potential is found to equal 0.87 V. Calculatethe concentration of Cr3+(aq) in the cell.
A 0.0712-g sample of a purified organic acid was dissolved in an alcohol-water mixture and titrated with coulometrically generated hydroxide ions. With a current of 0.0392 A, 241 s was required to reach aphenolphthalein end point. Calculate the equivalent mass of the acid.
Suppose Ered for Ag+Ag were set equal to zero instead of that of H+H2 . What would be (a) Ered for H+H2 ? (b) Eox for CaCa2+ ? (c) E° for the cell in 33(c)? Compare your answer with that obtained in 33(c).
Consider the following galvanic cells: For each galvanic cell, give the balanced cell equation and determine . Standard reduction potentials are found in Table 17-1.
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
Suppose Ered for H+H2 were taken to be 0.300 V instead of 0.000 V. What would be (a) Eox for H2H+ ? (b) Ered for Br2Br ? (c) E for the cell in 34(c)? Compare your answer with that obtained in 34(c).
A single HallHeroult cell (as shown in Fig. 17-22) produces about 1 ton of aluminum in 24 h. What current must be used to accomplish this?
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Zn|Zn2+(0.50M)Cd2+(0.020M)|Cd (b) Cu|Cu2+(0.0010M)H+(0.010M)|H2(1.00atm)|Pt