A galvanic cell is powered by the following redox reaction: 2+ 2 Zn(aq) + N₂H4(aq) + 4 OH (aq) → 2 Zn(s) + N₂(g) + 4H₂O(1) 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. = v 0-0 X

A galvanic cell is powered by the following redox reaction: 2+ 2 Zn(aq) + N₂H4(aq) + 4 OH (aq) → 2 Zn(s) + N₂(g) + 4H₂O(1) 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. = v 0-0 X

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 powered by the following redox reaction: 2+ 2 Zn²+(aq) + N₂H₂(aq) + 4OH¯(aq) → 2 Zn(s) + N₂(g) + 4H₂O(1) 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 0 E = V 00 S
Electrolysis of molten NaCl is done in a Downs cell operating at 7.0 volts and 4.0 x 10^4 A. How much Na (s) and Cl2 (g) can be produced in 4 hours in such a cell?
+ 2+ MnO 4(aq) +8 H (aq) +5e → Mn(aq) + 4H₂O(1) 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. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? 3+ If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to significant digits. Fe half-reaction 0 (aq) + e Yes No V 2+ Fe (aq) standard reduction potential red 'red = +1.51 V = +0.771 V ローロ x 90 x10 S
Please explain and give the correct answers.
A galvanic cell is powered by the following redox reaction: 2+ 2+ MnO₂ (s) + 4H* (aq) + Zn(s) Mn²+ (aq) + 2 H₂O(1) + Zn²+ (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 £ - Ov E V ローロ X G
Could you please solve the last two questions from the second picture?
A galvanic cell is powered by the following redox reaction: 2+ 2 Cro(aq) + 8 H₂O(1) + 3 Zn(s) 2 Cr(OH)3(s) + 10 OH¯(aq) + 3 Zn¹¹(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 □ E = v ロ→ロ e X Ś
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+ SnSO 4(aq) → NISO 4(aq)+ Sn(s) E1 E2 S1 S2
A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2NO(g) + 4H₂O(1) - 6 Br (aq) + 2NO3(aq) + 8H (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 00 Ś
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 voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 21 (aq) + Cl2(g) → 2(s) + 2CI(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate v the Cl2 electrode v the I electrode. Anions migrate v the salt bridge v the Cl2 compartment.
an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a Zn(NO3)2 solution. When a current of 1.95 A was used, it took exactly 1.7 hours to deposit a 0.0267-mm layer of zinc on the part. What was the total surface area of the part? The density of zinc is 7.410 g/cm^3. Assume the efficiency is 100%. Calculate your answer to at least 2 decimal places.