A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Cl₂(g)+2e 2 CI Write a balanced equation for the half-reaction that happens at the cathode. 2 103(aq)+ 12 H (aq) +10e Answer the following questions about this cell. 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 standard conditions? 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. O Yes O No 1 Ov I (aq) 4 1₂(s) + 6H₂O(1) standard reduction potential. V EO Ed=+1.195 V red ローロ e S 5

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Cl₂(g)+2e 2 CI Write a balanced equation for the half-reaction that happens at the cathode. 2 103(aq)+ 12 H (aq) +10e Answer the following questions about this cell. 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 standard conditions? 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. O Yes O No 1 Ov I (aq) 4 1₂(s) + 6H₂O(1) standard reduction potential. V EO Ed=+1.195 V red ローロ e S 5

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
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
Write the cell notation for an electrochemical cell consisting of an anode where Ni (s) is oxidized to Ni2+ (aq) and a cathode where Cu2+ (aq) is reduced to Cu (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
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 aluminum fluoride solution, AlF3(aq)
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 particular voltaic cell operates on the reaction below, giving an emf of 0.853 V. Calculate the maximum electrical work (in kJ) generated when 20.2 g of zinc metal is consumed. Zn(s) + CI2(g) → Zn2+(aq) + 2 Cl −(aq)
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)