Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. ローロ 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. E = [v %3D Round your answer to 2 decimal places. の

Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. ローロ 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. E = [v %3D Round your answer to 2 decimal places. の

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
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
A constant current of 0.50 A is used to deposit copper at the cathode and oxygen at the anode of an electrolytic cell. What is the weight of copper (63.55 g/mol) formed after 10 minutes? F=96,485 C
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2 IO3(aq)+12 H*(aq)+10e¯ 1₂(s) + 6H₂O(1) 2+ Cu²+ (aq)+e Cu (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. Do you have enough information to calculate the cell Yes 1 standard reduction potential = +1.195 V Ered red = +0.153 V
A galvanic cell is powered by the following redox reaction: + HNO₂(aq) + H+ (aq) + Cut ( Write a balanced equation for the half-reaction that takes place at the cathode. 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 anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. (aq) 0 2+ NO(g) + H₂O(1) + Cu²+ (aq) 0 E = V ローロ e
A certain half-reaction has a standard reduction potential Ed+0.57 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. red Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper Smit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at…
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
red A certain half-reaction has a standard reduction potential E = +0.16 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…
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A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
A galvanic (voltaic) cell contains a copper cathode immersed in a copper(I) chloride solution and a nickel anode immersed in a nickel(II) chloride solution. The two solutions are connected with a salt bridge. Write the balanced equation for the galvanic cell. Phases are optional. balanced equation: A current of 2.40 A is observed flowing through the cell for a period of 2.81 h. Calculate the amount of charge flowing through the circuit during this time. C Calculate the number of moles of electrons flowing through the circuit during this time. moles of clectrons: Calculate the mass change in grams of the copper and nickel electrodes. mass change of copper clectrodc: mass change of nickel electrode: