In the 1.0 M CUSO4 solution, the following species are present: Cu²+, SO42, H₂O, H3O+, and OH. Based on observed changes that occurred in each electrode, write the RHR, OHR, and the balanced overall reaction of electrolytic cell. The reactions should be consistent with the observations. For this part, refer to the following Setups: Electrodes Solution Current Time For the experimental data: Anode Carbon Setup 1 Initial mass of anode (g) Initial appearance of anode Final mass of anode (g) Observations at the anode Cathode Carbon 1.0 M CuSO4 1.50 A 20.00 minutes Table 8b-1. Data on the electrolysis of aqueous copper(II) Parameter Setup 1 14.02 Black-colored rod Anode Carbon Setup 2 1.0 M CuSO4 2.50 A 20.00 minutes 14.03 Part of electrode that was submerged became a little darker; bubble formation was observed during Cathode Carbon sulfate. Setup 2 13.85 Black-colored rod Setup 3 Anode Carbon Cathode Carbon 1.0 M CuSO4 1.50 A 30.00 minutes 13.85 Part of electrode that was submerged became a little darker; bubble formation was observed during Setup 3 15.15 Black-colored rod 15.16 Part of electrode that was submerged became a little darker; bubble formation was observed during

In the 1.0 M CUSO4 solution, the following species are present: Cu²+, SO42, H₂O, H3O+, and OH. Based on observed changes that occurred in each electrode, write the RHR, OHR, and the balanced overall reaction of electrolytic cell. The reactions should be consistent with the observations. For this part, refer to the following Setups: Electrodes Solution Current Time For the experimental data: Anode Carbon Setup 1 Initial mass of anode (g) Initial appearance of anode Final mass of anode (g) Observations at the anode Cathode Carbon 1.0 M CuSO4 1.50 A 20.00 minutes Table 8b-1. Data on the electrolysis of aqueous copper(II) Parameter Setup 1 14.02 Black-colored rod Anode Carbon Setup 2 1.0 M CuSO4 2.50 A 20.00 minutes 14.03 Part of electrode that was submerged became a little darker; bubble formation was observed during Cathode Carbon sulfate. Setup 2 13.85 Black-colored rod Setup 3 Anode Carbon Cathode Carbon 1.0 M CuSO4 1.50 A 30.00 minutes 13.85 Part of electrode that was submerged became a little darker; bubble formation was observed during Setup 3 15.15 Black-colored rod 15.16 Part of electrode that was submerged became a little darker; bubble formation was observed during

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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Calculate e values for the galvanic cells based on the following overall reactions. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm. (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLV2 References' Tables to answer this question as the values will not match.) Cr3+ (ag) + Cl2 (9) = Cr2 O,²- (aq) + Cl (ag) а. V b. Cu²+ (ag) + Mg(s) = Mg²+(aq) + Cu(s) V
N₂(g) + 4H₂O(1)+4e 3+ Fe (aq)+e Write a balanced equation for the half-reaction that 0 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 half-reaction nswer the following questions about this cell. information to calculate the cell voltage under standard conditions? 0 0 Yes No → Fe If you said it was possible to calculate the cell voltage, do so and enter your answer V 2+ (aq) N₂H₂(aq) +4 OH (aq) standard reduction potential E = +0.771 V 'red Eº 'red - 1.16 V ==
Subject :- Chemistry ...
eCovalentActivity.do?locator=Dassignment-take [Review Topics] [References] Use the References to access important values if needed for this question. Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) is oxidized to Mn+ (aq) and a cathode where Cr (aq) is reduced to Cr+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar. Retry Entire Group 8 more group attempts remaining Submit Answer
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction MnO4(aq) + 2 H2O(l)+3e MnO2(s)+4OH(aq) Br₂(1)+2e →>> 2 Br (aq) standard reduction potential E = +0.59 V 'red E = +1.065 V 'red Answer the following questions about this cell.
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