IS Consider a galvanic cell in which Alt is reduced to elemental aluminum and magnesium metal is oxidized to Mg2+, Write the balanced half-cell reactions that take place at the cathode and at the anode. half-cell reaction at the cathode: Al+3e → Al half-cell reaction at the anode:3 g (aq) + 6 e- Mg(s) 3 2+(aq)+6 e about us careers privacy policy terms of usE contact us help

IS Consider a galvanic cell in which Alt is reduced to elemental aluminum and magnesium metal is oxidized to Mg2+, Write the balanced half-cell reactions that take place at the cathode and at the anode. half-cell reaction at the cathode: Al+3e → Al half-cell reaction at the anode:3 g (aq) + 6 e- Mg(s) 3 2+(aq)+6 e about us careers privacy policy terms of usE contact us help

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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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
Consider a galvanic electrochemical cell constructed using Cr/Cr³+ and Zn/Zn²+ at 25 °C. The following half-reactions are provided for each metal: Cr³+(aq) + 3 e →→ Cr(s) E°red = -0.744 V Zn²+ (aq) + 2 e →→ Zn(s) Eºred = -0.763 V Write the balanced equation for the overall reaction in acidic solution. 3 Zn(s) + 2 Cr³+ (aq) → 3 Zn²+(aq) + 2 Cr (s) 1 1 + 4- Reset 2 H₂O+ 0 3_ ( ) 3 03 04 4 H H+ 5 5 11 Zn 6 6 ²+ 7 07 (s) H₂O ● 3+ (1) 8 9 0 e 4+ x H₂O 9 (g) (aq) □o Cr Delete
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
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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
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg²+(aq) → 2 Al3+(aq) + 3 Mg(s) 4.6E+31 9.0E-73 1.0E+24 1.1E+72 1.1E-72
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)