1. For an electrochemical cell at 25°C involving the oxidation of Cd to Cd2+ at one electrode and the standard hydrogen electrode as the other electrode: a. Write the half reaction at the anode. b. Write the half reaction at the cathode. c. Write the overall redox reaction. d. Is the cell a galvanic or electrolytic cell? Explain your answer. e. calculate AG° in kJ f. calculate K at 25°C g. calculate Ecell for [H+] = 0.058 M and [Cd2+] = 0.9 M

1. For an electrochemical cell at 25°C involving the oxidation of Cd to Cd2+ at one electrode and the standard hydrogen electrode as the other electrode: a. Write the half reaction at the anode. b. Write the half reaction at the cathode. c. Write the overall redox reaction. d. Is the cell a galvanic or electrolytic cell? Explain your answer. e. calculate AG° in kJ f. calculate K at 25°C g. calculate Ecell for [H+] = 0.058 M and [Cd2+] = 0.9 M

Chemistry

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter18: Electrochemistry

Section: Chapter Questions

Problem 133CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
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Consider the cell described below: Zn|Zn2+(1.00M)||Cu2+(l.00M)|Cu Calculate the cell potential after the reaction has operated long enough for the [Zn2+] to have changed by 0.20 mol/L. (Assume T=25C.)
Consider a cell based on the following half-reactions: a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate. b. When enough NaCl(s) is added to the compartment containing gold to make the [Cl] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that Au3+ is reduced and assume that the reaction in the compartment containing gold is Au3+(aq)+4Cl(aq)AuCl4(aq) Calculate the value of K for this reaction at 25C.
A standard galvanic cell is constructed so that the overall cell reaction is 2A13++(aq)+3M(s)3M2+(aq)+2A1(s) Where M is an unknown metal. If G = 411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the reaction proceeds spontaneously as written or spontaneously in the reverse direction under standard-state conditions. (a) H2(g)+Cl2(g)2H+(aq)+2Cl(aq) (b) Al3+(aq)+3Cr2+(aq)Al(s)+3Cr3+(aq) (c) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(s)
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Consider the galvanic cell based on the following half-reactions: a. Determine the overall cell reaction and calculate b. Calculate G and K for the cell reaction at 25C. c. Calculate at 25C when [Zn2+] = 0.10 M and [Fe2+] = 1.0 105 M.
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