+ ||TRED.of 36Consider these two entries from a fictional table of standard reduction potentials.X³+ +3e X(s)E° = -2.09 V%3DY³+ +3e Y(s)What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?cellTLF4F5F7F8F10F12PrtScrInsertDelete2$V.4.5.(7.Backsp80}{F.H.K.7.

Answered: Image /qna-images/answer/606359e9-56f5-4abb-b308-5c88c30c84d2.jpg

Consider these two entries from a fictional table of standard reduction potentials. X+ + 3e X(s) E° = -2.09 V %3D Y+ +3e → Y(s) E° = -0.25 V %3D What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? E° 'cell V

Consider these two entries from a fictional table of standard reduction potentials. X+ + 3e X(s) E° = -2.09 V %3D Y+ +3e → Y(s) E° = -0.25 V %3D What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? E° 'cell V

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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A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 Write the proper cell notation (with phases and concentrations) for the galvanic cell.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG^0 for the following redox reaction. 2Br-(aq) + 2H2O(l) -> Br2(l) + H2(g) + 2OH−(aq) Be sure your answer has the correct number of significant digitss
Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Nit] = 0.00170 M and [Au] = 0.868 M. Standard reduction potentials can be found in this table. %3D 3 Ni(s) + 2 Au*(aq) 3 Ni?+(aq) + 2 Au(s) E = V
Consider these two entries from a fictional table of standard reduction potentials. X+ (aq) + e¯ Y+ (aq) + e- →Y(s) E = 2.01 V →X(s) O X and Y O X+ and Y+ O X and Y+ O X+ and Y E = 2.62 V Which pair of species will react under standard conditions at 25 °C?
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy following redox reaction. Be sure your answer has the correct number of significant digits. H₂(g) + 2OH¯(aq) + 2Fe³+ (aq) → 2H₂O (1) + 2Fe²+ (aq) kJ x10 X Ś AGO for the
Consider the following standard reduction potentials: Zn2*(aq) + 2 e → Zn(s) E° = -0.76 V Mg2*(aq) + 2 e → Mg(s) E° = -2.37 V Ag*(aq) + e → Ag(s) E° = +0.80 V Which is the strongest oxidizing agent? Mg2*(aq) Zn2*(aq) Ag*(aq) 5:08 PM 90°F Partly sunny P Type here to search 8/6/2021
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ MnO2(s)+4H (aq)+2e → Mn (aq)+2 H₂O(1) 2+ Zn(aq) + 2e ->>> Zn(s) standard reduction potential E = +1.23 V red = -0.763 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. ☐ Do you have enough O Yes information to calculate the cell voltage under standard conditions? O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον ローロ e x10 ×
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Cu (aq)+e Cu (aq) = +0.153 V NO3 (aq)+4 H (aq)+3e NO(g)+2 H,O(1) E=+0.96 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough O Yes Explanation Check . Terms of Us 02022 McGraw Hill LLC. All Riahts Reserved. MAR étv 16