(a)
Interpretation:
The dependence of E in some half-cell reactions on pH should be explained.
Concept introduction:
In an
If oxidation takes place on an electrode, that electrode is called anode. The removal of electrons takes place from the species present in anode.
If reduction takes place on an electrode, that electrode is called cathode. The addition of electrons takes place to the species present in cathode. The electrode potential of cell is calculated from reduction electrode potential of cathode and anode as follows:
Nernst equation;
Z = number of moles of electrons transferred in the cell.
(b)
Interpretation:
Whenever H+ appears in a half-cell equation the reason for it to be on the left side should be explained.
Concept introduction:
In an electrochemical cell there are two electrodes that can be observed. Electrodes are named according to their tendency of oxidation or reduction.
If oxidation takes place on an electrode, that electrode is called anode. The removal of electrons takes place from the species present in anode.
If reduction takes place on an electrode, that electrode is called cathode. The addition of electrons takes place to the species present in cathode.
(c)
Interpretation:
Whenever OH- appears in a half-cell equation the reason for it to be on the right side should be explained.
Concept introduction:
In an electrochemical cell there are two electrodes that can be observed. Electrodes are named according to their tendency of oxidation or reduction.
If oxidation takes place on an electrode, that electrode is called anode. The removal of electrons takes place from the species present in anode.
If reduction takes place on an electrode, that electrode is called cathode. The addition of electrons takes place to the species present in cathode.
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General Chemistry: Principles and Modern Applications (11th Edition)
- Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .arrow_forwardConsider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?arrow_forwardTwo Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] = 1.0 105 M. When linked together with a salt bridge and external circuit, a cell potential is observed. (This kind of voltaic cell is referred to as a concentration cell.) (a) Draw a picture of this cell, labeling all components. Indicate the cathode and the anode, and indicate in which direction electrons flow in the external circuit. (b) Calculate the cell potential at 298 K.arrow_forward
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