Chapter 20, Problem 4
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?
Video transcript
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?
The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
(b) Is the electrode the anode or cathode?
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]
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+?
Consider the following voltaic cell:
(c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?
The electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc (b) Which battery do you think has an energy density most similar to the silver oxide battery: a Li-ion battery, a nickel– cadmium battery, or a lead–acid battery? [Section 20.7]