A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2 H₂O(1)+2e ->>> H₂(9)+2OH (aq) 3+ 2+ Fe2(aq) Fe (aq)+e → Fe (aq) 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 information to calculate the cell voltage under ☐ O Yes standard conditions? If you said it was possible to calculate the cell O No voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον E =-0.83 V red = +0.771 V red ローロ ē X G

A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2 H₂O(1)+2e ->>> H₂(9)+2OH (aq) 3+ 2+ Fe2(aq) Fe (aq)+e → Fe (aq) 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 information to calculate the cell voltage under ☐ O Yes standard conditions? If you said it was possible to calculate the cell O No voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον E =-0.83 V red = +0.771 V red ローロ ē X G

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

Suppose the galvanic cell sketched below is powered by the following reaction: 3 Mn(s)+2 Fe(NO3),(aq) 3 Mn(NO3),(aq)+2 Fe(s) E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. e Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? O OO OO O
Cro (aq) + 4 H₂O(1)+3e 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 swer the following questions about this cell. spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? 2+ Cu (aq) + e If you said it was possible to calculate the cell voltage, do so and enter your answer 0 half-reaction 0 2 Cu²+ (aq) + e → Cu (aq) Yes No + 0.28 V Cu (aq) Cr(OH)3(s)+5 OH (aq) standard reduction potential E .0 'red Eº ´red = +0.153 V -0.13 V ロ→ロ e × x10 Ś
G ロ・ロ A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ MnO2 (s) + 4H* (aq) +2Cr²* (aq) → Mn²* (aq) + 2H2O (1) +2Cr³+ (aq) Suppose the cell is prepared with 0.190 M H* and 6.41 M Cr²+ in one half-cell and 0.205 M Mn2+ and 1.94 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ ☐ x10 μ
A chemist designs a galvanic cell that uses these two half-reactions: 2 H₂O(1)+2e 2+ Zn² (aq) +2e 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. Answer the following questions about this cell. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough half-reaction information to calculate the cell voltage under standard conditions? significant digit 0 0 Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer ☐V here. Round your answer to 1 H₂(g) + 2 OH (aq) Zn(s) standard reduction potential Eº red Eve 'red 0.83 V == - 0.763 V ロ→ロ X 90 x10
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
Lab 5 8-6: Friedel-Crafts-3 For this amignient, the turget compound that you sbould syathesite is 2-methyt-benophenone. This is an electrophilie arcmatie, substitution resction Eaamine the prodact carefully and determine the substination pattern. Which groep will aiready be present in the substrate Keep in mind the mechanism and bow that will control the selectivity of the proces Remember, you can casily separate ortho and para Isomers Synthesis Procedures 1. Start Virtunl Chemlah and select Friedel-Crafts -3 from the list of assignments on the whiteboard. Afler catering the synthesis laboratory, use the available reagents on the stockroom shelf and identify the appropriate starting materials required to nynthesize the target compound and add them to the round bottom flask. Select the appropriate solvent and drag the flask to the Stir Plate on the lab bench. 2. The round bottom flask containing the starting materials should now be on the stir plate, and the contents of the flask ahould…
A galvanic cell is powered by the following redox reaction: 2+ 2 Cu²+ (aq) + H₂(g) + 2OH¯(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 □ 0 E = v + 2 Cu (aq) + 2 H₂O(1) ロ→ X Ś
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
signs a galvanic cell that uses these two half-reactions: half-reaction 2 H₂O(1)+2e H₂(g) + 2OH(aq) 3+ 2+ Fe³+ (aq)+e → Fe²+ (aq) 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. A chem standard reduction potential E-0.83 V red E 'red = +0.771 V 2H₂O(1) + 2e → H₂(g) + 2OH(aq) 2+ 3+ Fe → Fe (aq) + e 7 ロ→ロ e X x10 Ś ?
What reactions take place at the cathode and the anode when each of the following solutions is used in an electrolytic cell? Write the half-reaction equations for the anode and cathode, and state whether the reaction would result in metal being plated onto the object. 1.0 mol/L manganese iodide solution, Mn12(aq)