Electrolytic cellSetup 1Setup 2Setup 3AnodeCathodeAnodeCathodeAnodeCathodeElectrodesCarbonCarbonCarbonCarbonCarbonCarbonSolutions1.0 M CuSO41.0 M CuSO41.0 M CuSO4Current1.50 A2.50 A2.50 ATime10.00 minutes10.00 minutes15.00 minutesIn the 1.0 M CuSO4 solution, the following species are present: Cu2+, SO4 2- , H2O, H3O+, and OH- .Based on the observed changes that occurred in each electrode, write the RHR, OHR, and the balancedoverall reaction of the electrolytic cell. The reactions should be consistent with the observations.

Answered: Image /qna-images/answer/19ba30ce-fe58-4a9d-bf00-ffda92cd6624.jpg

Electrolytic cell Setup 1 Setup 2 Setup 3 Anode Cathode Anode Cathode Anode Cathode Electrodes Carbon Carbon Carbon Carbon Carbon Carbon Solutions 1.0 M CuSO4 1.0 M CuSO4 1.0 M CuSO4 Current 1.50 A 2.50 A 2.50 A Time 10.00 minutes 10.00 minutes 15.00 minutes In the 1.0 M CuS04 solution, the following species are present: Cu2+, SO4 2- , H2O, H3O+, and OH- . Based on the observed changes that occurred in each electrode, write the RHR, OHR, and the balanced overall reaction of the electrolytic cell. The reactions should be consistent with the observations.

Electrolytic cell Setup 1 Setup 2 Setup 3 Anode Cathode Anode Cathode Anode Cathode Electrodes Carbon Carbon Carbon Carbon Carbon Carbon Solutions 1.0 M CuSO4 1.0 M CuSO4 1.0 M CuSO4 Current 1.50 A 2.50 A 2.50 A Time 10.00 minutes 10.00 minutes 15.00 minutes In the 1.0 M CuS04 solution, the following species are present: Cu2+, SO4 2- , H2O, H3O+, and OH- . Based on the observed changes that occurred in each electrode, write the RHR, OHR, and the balanced overall reaction of the electrolytic cell. The reactions should be consistent with the observations.

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

For an electrochemical cell, the reduction potential for the anode and the cathode are 0.287 V and 0.698 V, respectively. What is the overall cell voltage for this system? O +0.411 V O -0.411 V O +0.698 V O +0.287
Draw the galvanic cell from the following half-reactions (use KCl as salt bridge) Al3 + aq + 3rd → Als Ni2 + aq + 2é → Ni (s) Indicates the anode and cathode Indicates where oxidation and reduction occur Indicates the direction of movement of electrons. Indicates the direction of movement of the ions. Write the balanced ionic equation of this equation
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…
Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell V
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
Suppose you set up an electrochemical cell. In one beaker, you have a 1 M copper(I) ion solution with a copper metal electrode. You use an external wire to connect the cop electrode to an aluminum electrode in another beaker with a 1 Maluminum lon solution. Then you add a salt bridge with sodium sulfate ions. All things are in place to have functional cell. Which of the following statements is FALSE? Nothing will happen until you add an external power source. Without a power source, electrons will travel from the aluminum beaker to the copper beaker You can run this as a voltaic cell and get out a maximum of 2.00 V You can run this as an electrolytic cell only if you input a minimum of 2.00v
Cell Potential For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: Ecell Ered (cathode) - Ed (anode) ▼ Tarnish on copper is the compound CuO. A tarnished copper plate i placed in an aluminum pan of boiling water. When enough salt is added so that the solution conducts electricity, the tarnish disappears. Imagine that the two halves of this redox reaction were separated and connected with a wire and a salt bridge. Part A Calculate the standard cell potential given the following standard reduction potentials: A²+ +3e Cu²+ + 20 Express your answer to two decimal places and include the appropriate units. ▸ View Available Hint(s) Ecell = li Value 4 → Units ? Al; E Cu; E 19 of 42 -1.66 V 0.340 V Review | Constants | Periodic Table
6. Electrolysis of water using platinum electrode produces oxygen gas at the anode and hydrogen gas at the cathode according to the following half-cell reactions. Anode: 2H20 → 02 + 4H* + 4e Cathode: 4H20 + 4e → 2H2 + 40H- Determine the mass of hydrogen gas that are liberated after 5mins wit a current of 0.2 A. Given atomic mass of hydrogen, H is 1 g/mol, 1 Faraday = 96500 C/mol e
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ MnO₂(s)+4H(aq) +2e → Mn(aq) + 2 H₂O(1) Zn²+ (aq)+2e Zn(s) Answer the following questions about this cell. standard reduction potential E=+1.23 V red E =-0.763 V red
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. 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? 0 0 0 0 0 0
Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.