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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What to do: Read each statement below and identify if it defines electrode potential, reduction potential, oxidation potential or cell potential. Write your answers on a separate sheet of раper. 1. It refers to the difference of equilibrium potential between the surrounding solution and the metal electrode. 2. It is the reaction that takes place at the cathode. 3. It is the reaction that takes place at the anode. 4. It is the ability of anion solution to become reduced picking up or gaining electrons from its own electrode. 5. It is the ability of an electrode to become oxidized giving up or losing electrons. 6. It refers to the potential difference between the electrodes corresponding to an external electron flow from anode to cathode. 7. It is the combination of reduction potential at the cathode and oxidation potential at the anode. 8. An example of this reaction is Zns) 9. An example of this reaction is Cu*?laq) + 2e- 10. It is illustrated as: Ecell = Eox,Anode + Ered,Cathode Znag)…
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 =
Define voltaic cell.
If the given statement is true, write T. Otherwise, write F and explain why it is false 1)An electrolytic cell is used to generate electricity from chemical reactions 2) The reactant and the product need to have equal concentrations for a chemical reaction to be in equilibrium.
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
Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl solution - a Ni electrode in 1.0 M Ni(NO) solution When the cell is running spontaneously, which of the choices are true? a.) The nickel electrode gains mass and the nickel electrode is the cathode. b.) The nickel electrode loses mass and the nickel electrode is the cathode. c.) The iron electrode gains mass and the iron electrode is the anode. d.)The iron electrode loses mass and the iron electrode is the cathode.
one of the differences between a voltaic cell and an electrolyte cell is that in an electrolyte cell this happens (see image)
Draw a diagram of an electrochemical cell. Use iron and silver for the electrodes. Include and label electrodes, electrolyte, cathode, anode, and the direction of electron flow.
You are a bioengineer designing a new type of pacemaker. Which type of Galvanic cell would be best for you to use in this new device?
What reaction (oxidation or reduction) occurs at the cathode of a voltaic cell? What is the sign of the cathode? Do electrons flow toward or away from the cathode?
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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