### Galvanic Cell DesignA chemist designs a galvanic cell that uses these two half-reactions:| Half-Reaction | Standard Reduction Potential || --- | --- || \( \text{CrO}_4^{2-}(\text{aq}) + 4 \text{H}_2\text{O}(l) + 3e^- \rightarrow \text{Cr(OH)}_3(s) + 5 \text{OH}^- (\text{aq}) \) | \( E^\circ_{\text{red}} = -0.13 \text{ V} \) || \( \text{Zn}^{2+} (\text{aq}) + 2e^- \rightarrow \text{Zn}(s) \) | \( E^\circ_{\text{red}} = -0.763 \text{ V} \) |#### Questions:1. **Write a balanced equation for the half-reaction that happens at the cathode.** \[ \boxed{} \]2. **Write a balanced equation for the half-reaction that happens at the anode.** \[ \boxed{} \]3. **Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.** \[ \boxed{} \]4. **Do you have enough information to calculate the cell voltage under standard conditions?** - ☐ Yes - ☐ No5. **If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits.** \[ \boxed{\text{ V}} \]### Explanation of DiagramA diagram on the right-hand side likely represents the electronic configuration or the movement of electrons involved in the redox reactions. It contains small square boxes indicating electrons (\( e^- \)) arranged in patterns. However, further analysis of this diagram requires specific context provided in the accompanying materials which isn't detailed here.

1. At cathode reduction occure and have higher standard reduction potential. 2. At anode oxidation…

Cro²(aq)+4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Zn²+ (aq)+2e → Zn(s) swer 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 standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 0 0 0 O Yes half-reaction O No ☐v standard reduction potential -0 red red = -0.13 V =-0.763 V ローロ e X 1. x1

Cro²(aq)+4H₂O(1)+3e¯ Cr(OH)3(s)+5 OH(aq) Zn²+ (aq)+2e → Zn(s) swer 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 standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. 0 0 0 O Yes half-reaction O No ☐v standard reduction potential -0 red red = -0.13 V =-0.763 V ローロ e X 1. x1

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

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
Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 14 minutes at a current of 2.3 A given the following reaction. Z3+(aq) + 3e- → Z(s) Atomic Mass: Z: 176.56 g/mol
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
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
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
A galvanic cell is powered by the following redox reaction: MnO (aq) + 2 H₂O(1) + 3 Cut (aq) ► MnO₂ (s) + + 4 OH (aq) + 3 Cu²+ (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
Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized to Cr** (aq) and a cathode where Co2+ (aq) is reduced to Co (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
write the half-reactions that occur at the anode and cathode during the electrolysis of NH4Cl in aqueous solution.
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