A galvanic cell is powered by the following redox reaction: MnO4(aq) + 8 H* (aq) + 5 Cu* (aq) → Mn²+ (aq) + 4H₂O(l) + 5 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 = OV ローロ e™ X

A galvanic cell is powered by the following redox reaction: MnO4(aq) + 8 H* (aq) + 5 Cu* (aq) → Mn²+ (aq) + 4H₂O(l) + 5 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 = OV ローロ e™ 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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+ 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
The two half cells that make up a battery are shown below with their reduction potentials: Br2(aq) + 2e → 2B1¯(aq); E= 1.07 V Cu²+(aq) + e – Cu*(aq); E= 0.16 V What is the equation for the galvanic cell made with these two half equations? Oa. 2Cu*(aq) + Br2(aq) – 2Cu2+(aq) + 2Br (aq) Ob. 2Cu2*(aq) + Br2(aq) → 2Cu*(aq) + 2Br"(aq) Oc. 2Cu*(aq) + 2Br (aq) – 2Cu²* (aq) + Br2(aq) Od. 2Cu2*(aq) + 2B1°(aq) → 2Cu*(aq) + Br2(aq) Oe. None of the other options
A galvanic cell is powered by the following redox reaction: Br,(1) + H,(g) + 2 OH (aq) - 2 Br (aq) + 2 H,O(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. O-0 Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = [y Round your answer to 2 decimal places. Explanation Check O 2022 McGraw Hill LLC. All Riahts Reserved. Terms of Use F étv 17
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
Calculate the cell potential given the standard reduction potentials for the half reactions of the following hypothetical elements: X3+(aq) + e- → X2+(aq) SRP: +0.57 V Y2(ℓ) + 2e- → 2Y-(aq) SRP: +0.41 V
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
A galvanic cell is powered by the following redox reaction: Cl₂(g) + 2NO(g) + 2 H₂O(1) → 2 CI (aq) + 2 HNO₂(aq) + 2H¹ (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. E = v ローロ e