The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The cell operates according to the reaction represented by the following equation. Zn (s) + Ni2+ (aq) → Ni (s) + Zn²+ (aq) Salt Bridge in SO X2+ SO a. Identify M and M²+ in the diagram and specify the initial concentration for M²+ in solution. b. Indicate which of the metal electrodes is the cathode. Write the balanced equation for the reaction that occurs in the half-cell containing the cathode. c. What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 Min the half-cell containing the Zn electrode? d. Describe what would happen to the cell voltage if the salt bridge was removed. Explain.

The diagram below shows the experimental setup for a typical electrochemical cell that contains two standard half-cells. The cell operates according to the reaction represented by the following equation. Zn (s) + Ni2+ (aq) → Ni (s) + Zn²+ (aq) Salt Bridge in SO X2+ SO a. Identify M and M²+ in the diagram and specify the initial concentration for M²+ in solution. b. Indicate which of the metal electrodes is the cathode. Write the balanced equation for the reaction that occurs in the half-cell containing the cathode. c. What would be the effect on the cell voltage if the concentration of Zn2+ was reduced to 0.100 Min the half-cell containing the Zn electrode? d. Describe what would happen to the cell voltage if the salt bridge was removed. Explain.

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

An electrochemical cell has the following cell notation:Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) a. Write a balanced equation for the overall reaction. b. Determine the potential, E, for this cell at 298 K when [Ni2+] = 0.00200 M and [Al3+] = 0.500 M. c. Is the reaction in part (b) spontaneous or nonspontaneous?
For each redox reaction, write the half-reactions and draw the cell diagram for a galvanic cell (use short hand cell notation) in which the overall reaction occurs spontaneously. Identify each electrode as either positive or negative. a. Ag(s) + Fe3+ (aq) → Ag+ (aq) + Fe2+ (aq)
1. Sketch an electrochemical cell that uses the given reaction. Label the anode and cathode; indicate the direction of electron flow; write a balanced equation for the cell reaction; and calculate E°cell, AG° and K. NO3^- (aq) + H^+(aq) + Zn(s) -> Zn^2+ (aq) + NO(g) + H20(l) 2. The given cell reaction is spontaneous at standard state. True or False? 3. Which is favored by the cell reaction? Reactants or Products?
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + Enter the reaction that takes place at the cathode. Include state symbols: + In the external circuit, electrons migrate v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to
Calculate the cell potential for the reaction as written at 25.00 degrees * C , given that [Zn^ 2+ ]=0.81 and [Sn^ 2+ ]=0.0190M M. Use the standard reduction potentials in this table. Zn(s)+ Sn ^ 2+ (aq) rightleftharpoons Zn^ 2+ (aq)+Sn(s)
Answer the following questions using the data in Appendix L of the textbook. a. Calculate the standard cell potential for a galvanic cell made with Ni and Ag. b. Calculate the standard cell potential for a galvanic cell made with Ni and Zn.
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
A galvanic cell is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2 Br¯ (aq) → Mn²(aq) + 2 H₂O(1) + Br₂(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. 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 ローロ 0
Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.
A voltaic cell is constructed with a Ni//Ni2+ half-cell and a Ag/Ag+ half-cell. The nickel electrode is negatively charged. Draw a diagram of the cell, labeling the electrodes with their charges and showing the direction of electron flow in the circuit and of cation and anion flow in the salt bridge.Identify the anode and cathode half-reactions and show the shorthand notation. Calculate the standard potential in volts for the reaction at room temperature
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
2+ Consider an electrochemical cell made up of Cu Cu²+ and Ag | Agt half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E £º =0 ロ→ロ V 2+ Calculate the standard emf of a cell that uses the Cu Cu²+ and Ag | Ag* half-cell reaction at 25 °C. Round your answer to 3 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. X ปี x10 Ś X Ś