(a)
Interpretation:
The electrode reactions and the net cell reaction for Zn − Br2 potential battery system should be described. The theoretical voltage of the battery should be determined.
Concept introduction:
Battery is a device that store chemical energy in order to release later as electricity. Batteries may consist of single voltaic cell with two electrodes or may contain two or more voltaic cells linked in series.
(b)
Interpretation:
The electrode reactions and the net cell reaction for Li − F2 potential battery system should be described. The theoretical voltage of the battery should be determined.
Concept introduction:
Battery is a device that store chemical energy in order to release later as electricity. Batteries may consist of single voltaic cell with two electrodes or may contain two or more voltaic cells linked in series.
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Selected Solutions Manual For General Chemistry: Principles And Modern Applications
- You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell potential will be close to (a) 1.1 V and (b) 0.50 V. Consider cells in which the zinc cell can be either the cathode or the anode.arrow_forwardFor a voltage-sensitive application, you are working on a battery that must have a working voltage of 0.85 V. The half-cells to be used have a standard cell potential of 0.97 V. What must be done to achieve the correct voltage? What information would you need to look up?arrow_forwardConsider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?arrow_forward
- The following half-cells are available: (i) Ag+(aq, 1.0M)|Ag(s) (ii) Zn2+(aq, 1.0 M) |Zn(s) (iii) Cu2+(aq, 1.0M)|Cu(s) (iv) Co2+(aq, 1.0M)|Co(s) Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag-Zn, Ag-Cu, Ag-Co, Zn-Cu, Zn-Co, and Cu-Co. (a) In which of the voltaic cells does the copper electrode serve as the cathode? In which of the voltaic cells does the cobalt electrode serve as the anode? (b) Which combination of half-cells generates the highest potential? Which combination generates the lowest potential?arrow_forwardCalculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.015 M. 2 Fe2+(aq) + H2O2(aq) + 2 H+(aq) 2 Fe3+(aq) + 2 H2O()arrow_forwardThe standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.arrow_forward
- Consider the cell Pt|H2|H+H+|H2|Pt In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except that the solution around the platinum electrode has a pH of 0.0. What is the cell voltage?arrow_forwardConsider 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_forwardFor the ?G values given here, determine the standard cell potential for the cell.. (a) 12kJ/mol,n=3 (b) 45kJ/mol,n=1arrow_forward
- Balance the following reactions and write the reactions using cell notation. Ignore any inert electrodes, as they are never part of the half-reactions. (a) Al(s)+Zr4+(aq)Al3+(aq)+Zr(s) (b) Ag+(aq)+No(g)Ag(s)+NO3(aq) (acidic solution). (C) SiO32(aq)+Mg(s)Si(s)+Mg(OH)2(s) (basic solution). (d) CIO3(aq)+MnO2(s)CI(aq)+MnO4(aq) (basic solution)arrow_forwardConsider the cell described below: Al|Al3+(1.00M)||Pb2+(1.00M)|Pb Calculate the cell potential after the reaction has operated long enough for the [Al3+] to have changed by 0.60 mol/L. (Assume T = 25C.)arrow_forwardFor each of the following electrochemical cells, write equations for lire oxidation and reduction half-reactions and for the overall reaction (a) Pb(s)|Pb2+(aq)||Sn4+(aq),Sn2+(aq)|C(s) (b) Hg()|Hg2Cl2(s)|Cl(aq)||Ag+(aq)|Ag(s)arrow_forward
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