RubricAnswer the question below. View the rubric linked above for help if needed.Analyze the following diagram of a voltaic cell. Explain the structure and function of its components, the reactions occurring within it, and its overall purpose. Your answer should include the following vocabulary: anode, cathode,electrons, oxidation, reduction, redox, salt bridge, and electric current. Use details to support your answer.SnNO, salt bridge K+Na,50PbNO,Sn35m² +NOSn²+NO2-Pb 50,-Sn2+NO Sn²+SO-2-NO-SO-PSn2+NO,K+Sn²+NO, Sn²+tin nitrate solutionSn²+SO2-SO, SO-SO2-K+ SO2-lead sulfate solutionBiU Font Family- AA▾ ADFE EC医↓ tv1 Very high pollenDPrevious7 of 15NextSave & exit1:44 PMAll changes sa

Components of the Voltaic Cell Anode and Cathode:Anode: The anode is where oxidation occurs. In this…

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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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Explain the process of electrolysis using the diagram below. Where does oxidation occur? Where does reduction occur? Describe the direction of the flow of electrons. How is this electrolytic cell different from a voltaic cell? Note: The symbol Me stands for a metal. Show all work and answer in complete sentences.
Write half-reaction for the cell's cathode. Include the phases of all species in the chemical equation.
Give two suggestions to prevent corrosion Name two differences between galvanic (voltaic) cells and electrolytic cells. What is corrosion? Define and give an example
All of the following statements regarding electrochemical cells are true except All electrochemical cells require an applied electric current. In a voltaic cell the electrons flow from the anode to the cathode. In a voltaic cell, the half reactions are separated. The salt bridge maintains electricalcontact and charge neutrality.
A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H (aq) +Se Fe³+ (aq) +e 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. half-reaction Write a balanced. equation for the Answer the following questions about this cell. 0 - Mn² (aq) + 4H₂O(1) Fe (aq) standard reduction potential +1.51 V Ered=+0.771 V 20 "red =
1) How are the terms “electrochemical cell” and “battery” related? 2) Give a brief description of how and why a battery works. 3) There are two types of batteries: Primary and secondary. How are these types of batteries different from one another? How are they the same?
Define voltaic cell.
Analyze the components of a voltaic electrochemical cell. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Hg2+(aq) + Cu(s)→ Hg(I) + Cu²+(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 to v the Hg+ electrode from v the Cu electrode. In the salt bridge, anions migrate to the Cu compartment [from v) the Hg compartment.
Completely analyze the following electrolytic cell. Note that the electrodes are not inert and because of that, the anode might oxidize. Cu Anode Reaction Cathode Reaction Chemicals produced at the anode Chemicals produced at the cathode The electrons flow from Which electrode is the anode ? Power Source 1 M NaF (aq) + Cu
Design an experiment to measure the standard potential of a Silver Describe your electrochemical cell in detail, including the setup, the chemical reactions and notation. \Write up your experiment in such a way that a chemist can carry out your instructions).

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