Match each of the following components of an electrochemical cell: Transports electrons between half cells Site of oxidation Ensures that the two different redox conjugate pairs remain separated Site of reduction Maintains charge balance Salt bridge Power cord Redox conjugate pair Anode Cathode Porous plug Wire (external circuit)

Match each of the following components of an electrochemical cell: Transports electrons between half cells Site of oxidation Ensures that the two different redox conjugate pairs remain separated Site of reduction Maintains charge balance Salt bridge Power cord Redox conjugate pair Anode Cathode Porous plug Wire (external circuit)

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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All products in half-cell reactions can be changed back into its original reactants.Group of answer choices True False
Consider a voltaic cell comprised of Zn/Zn2+ at one electrode and Fe2*/Fe3+ at the other electrode at standard conditions. Electrons will flow from the [ Select ] , which is the [ Select ] , and the cations in the salt bridge will flow towards the [Select ] . You may find a list of standard reduction potentials useful.
Which of the following statements are true about the cathode during the operation of a voltaic electrochemical cell? © Metal cations can deposit as the corresponding metal on the surface of the cathode The cathode is positively charged with respect to the anode. The cathode is where the reduction reaction occurs. In a salt bridge, the positively charged ions flow towards the cathode. Onlv two of the above four statements are true Only three of the first four statements above are true. All of the first four statements above are true.
For a voltaic cell based on the reaction below, what reaction happens at the cathode?Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) Zn(s)→Zn2+(aq)+2e- 2H+(aq)+2e-→H2(g) Zn2+(aq)+2e-→Zn(s) H2(g)→2H+(aq)+2e-
if the following electrochemical cell is in operation: a) Nitrate ions (NO3-) migrate towards half of the copper cell b) Copper (II) ions (Cu2 +) migrate through the salt bridge c) magnesium ions (Mg2 +) migrate through the salt bridge d) potassium ions (K +) migrate towards the half-magnesium cell
When creating an electrochemical cell, why is it important to prevent the reactants from any direct contact?
Fully label the unlabelled Galvanic cell below using the following information: Electrodes: Magnesium and Zinc Salt Bridge: KNO3 a- Identify the anode and cathode (and the solution each is in) b- Write the anode and cathode half-cell reactions c- Write the overall cell reaction d- Show the direction of e- flow e- Show the direction of ion flow in the salt bridge f- Predict which electrode will increase in mass and which electrode will decrease in mass. Explain your answer.
In Electrochemical cells electrons are transfered from the reactants being reduced to the reactants being oxidized through a wire connecting the two containers. (True/False)
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.
When electrochemical cells are used as chemical probes, equilibrium between the half-cells must be established. O True O False
Zinc II Sulfate & Aluminum Chloride Half – Reaction in anode: Half- Reaction in cathode: Balanced cell reaction
Select all the statements below that are always true with respect to electrochemical cells: Oxidation occurs at the anode The free electrons in solution assist in maintaining the charge imbalance Electron flow occurs spontaneously Reduction occurs at the cathode Electrons move through a wire that connects the two half-cells The species that loses electrons is reduced The species that loses electrons is oxidized A salt bridge is required to preserve electric neutrality The side that loses electrons becomes increasingly positive An inert electrode is necessary