An Aluminium-Air Battery Al9 / AlPr(@«) // H2O@/Oz@/ C¢9 Wire Granular Carbon Damp Paper Towel Sheet of Aluminium The aluminium-air battery shown above is made out of aluminium foil, a paper towel soaked in an electrolyte solution and ground up charcoal. In theory, you only need water for the cell to work but an electrolyte like sodium chloride or potassium hydroxide will improve its performance. Under standard conditions, one cell of the aluminium-air battery would have an electrical potential of v.

An Aluminium-Air Battery Al9 / AlPr(@«) // H2O@/Oz@/ C¢9 Wire Granular Carbon Damp Paper Towel Sheet of Aluminium The aluminium-air battery shown above is made out of aluminium foil, a paper towel soaked in an electrolyte solution and ground up charcoal. In theory, you only need water for the cell to work but an electrolyte like sodium chloride or potassium hydroxide will improve its performance. Under standard conditions, one cell of the aluminium-air battery would have an electrical potential of v.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 115AE: The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making...

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The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Consider 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?
Sketch a galvanic cell, and explain how it works. Look at Figs. 17-1 and 17-2. Explain what is occurring in each container and why the cell in Fig. 17-2 works but the one in Fig. 17-1 does not.
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, .
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?