(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-MOD.MASTERINGCHEM.
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- Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?arrow_forwardA galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.arrow_forwardConsider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).arrow_forward
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