Skip to main content
Pearson+ LogoPearson+ Logo
Ch.20 - Electrochemistry
All textbooksBrown 15th EditionCh.20 - ElectrochemistryProblem 3b
Previous problem
Next problem
Chapter 20, Problem 3b

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
Molecular view of a process at an electrode in a voltaic cell, showing electron movement.


(b) Is the electrode the anode or cathode?
Close-up of molecular interactions at an electrode in a voltaic cell, illustrating electron transfer.

Verified step by step guidance
1
Identify the process occurring at the electrode by analyzing the molecular view. Notice that atoms are leaving the electrode surface, indicating a loss of material.
Recognize that the loss of atoms from the electrode surface suggests oxidation, as atoms are losing electrons and becoming ions.
Recall that in a voltaic cell, oxidation occurs at the anode. Therefore, the electrode where atoms are leaving must be the anode.
Confirm that the electrode is the anode by noting that oxidation (loss of electrons) is taking place, which is consistent with the behavior of an anode in a voltaic cell.
Conclude that the electrode depicted in the molecular view is the anode, as it is the site of oxidation where atoms are losing electrons and becoming ions.

Verified Solution

Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?
Previous problem
Next problem
Related Practice
Textbook Question

A voltaic cell is constructed that uses the following half-cell reactions:

Cu+(aq) + e- → Cu(s)

I2(s) + 2 e- → 2 I-(aq)

The cell is operated at 298 K with [Cu+] = 0.25 M and [I-] = 0.035 M.

(b) Which electrode is the anode of the cell?

(c) Is the answer to part (b) the same as it would be if the cell were operated under standard conditions?

Textbook Question

In the Brønsted–Lowry concept of acids and bases, acid– base reactions are viewed as proton-transfer reactions. The stronger the acid, the weaker is its conjugate base. If we were to think of redox reactions in a similar way, what particle would be analogous to the proton? Would strong oxidizing agents be analogous to strong acids or strong bases? [Sections 20.1 and 20.2]

1060
views
Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

(a) Does the process represent oxidation or reduction?

635
views
Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

(c) Why are the atoms in the electrode represented by larger spheres than those in the solution? [Section 20.3]

627
views
Textbook Question

Assume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water.

(a) What additions must you make to the cell for it to generate a standard emf?

660
views
Textbook Question

Consider the following table of standard electrode potentials for a series of hypothetical reactions in an aqueous solution: reduction half-reaction E °(V) (c) Which substance(s) can oxidize C2+?

1173
views