VISUALIZATIONA Voltaic Electrochemical CellVoltmeterAnodeCathodewireSalt bridgeAnodeCathode(-)alt brid(+)Oxidation-reduction reactions are different from all other types of reactions in that these reactions can be made to take place with the two reactants not coming into direct contact with each other. This is accomplished using an electrochemical cell, wherethe two reactants are placed in separate compartments and connected using a wire and a "salt bridge." Examine the cell shown here and watch the animation, then answer the questions that follow.What type of reaction occurs at the cathode?O oxidationO reductionSubmit(PreviousNext What type of reaction occurs at the anode?O oxidationO reductionSubmitIn which direction do electrons flow through the wire?O from anode to cathodefrom cathode to anodeSubmitIn which direction will anions flow relative to the salt bridge?from the anode compartment into the salt bridgeO from the cathode compartment into the salt bridgeSubmit

In general,in a galvanic(voltaic) cell, the electrode at which reduction takes place is written on…

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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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O ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2+ Fe (aq) Ed=+0.771 V %3D 3+ red Fe"(aq)+e Cro (aq)+4 H,O(1)+3e Cr(OH),(s)+5OH (aq) -0.13 V Ered nswer the following questions about this cell. Jrite a balanced quation for the alf-reaction that appens at the athode. rite a balanced uation for the If-reaction that ppens at the ode. ite a balanced uation for the erall reaction
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 =
When creating an electrochemical cell, why is it important to prevent the reactants from any direct contact?
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.
The diagram below is an electrochemical cell based on a redox reaction that needs to be completed by a student in the laboratory. Zn(s) + Br₂(1)→ Zn²+ (aq) + 2 Br¯(aq) C electron flow? B H Salt Bridge Gr Zn mm F What is the overall voltage of the cell? Wrie your answer to 3 significant figures in volts. Do not include units in your answer.
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
Which of these is a function of a salt bridge in an electrochemical cell? O It permits the charges to stay unbalanced in the two half-cells. O It does not allow migration of ions between the solutions. O It connects the two half-reactions. O It forces the electrons to travel through the inner circuit.
In each , decide whether the property measured was a chemical or physical property of X, if you can. If you don't have enough information to decide, choose can't decide in the third column. property R V H experiment Into one chamber of an electrochemical cell, a solution of X is introduced, along with a metal electrode. In the other chamber a solution of a known oxidizing reagent O is introduced, along with another metal electrode. The voltage across the electrodes is proportional to the tendency of O to react with X. By measuring this voltage, the value of R may be calculated. A sample of X is melted and put into a reservoir from which a very thin tube leads down. The rate at which X flows out of the tube is measured, and from this rate the value of V may be calculated. A sample of X is carefully weighed and put inside a sealed calorimeter. The calorimeter is heated electrically, and the amount of heat added determined by monitoring the electrical current used. The temperature of X is…
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).
A student mistakenly puts the opposite reactants into a voltaic cell, then uses a voltmeter to measure the voltage. What will happen? There could be sparks flying and possible fire or worse. No reaction will happen. The student may experience an electrical shock. The measured voltage will be negative.
It is known that at both electrodes of the voltaic cell there is an acid solution that produces hydrogen gas at the anode and cathode. The flow of electrons flows from a concentration of 0.05 M to a higher concentration of 0.5 M. If the rods at the anode and cathode are platinum (Pt), then the voltaic cell potential measured on the voltmeter is ... A. 0.5092 V B. 0.1184 V C. 0.1776 V D. 0.0592 V

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