Question 1 (1 point) An electrochemical cell is set up with a Cu(s)|Cu(NO3)2(aq) electrode (E° red = +0.34 V) and an Ag(s)|Ag(NO3)(aq) electrode (E° red = +0.80 V). Select the FALSE statement(s) concerning the operation of this cell: i) The concentration [Cu2+] decreases in the Cu half-cell. ii) The Ag electrode gains mass during operation of teh cell. iii) Cu metal is less easily oxidized than Ag metal. iv) The mass of the Cu electrode decreases during operation of the cell. v) Silver ions migrate from the Ag half-cell to the Cu half-cell through the salt bridge. i, iii, v ii, iv i, v ii, iii, iv all

Question 1 (1 point) An electrochemical cell is set up with a Cu(s)|Cu(NO3)2(aq) electrode (E° red = +0.34 V) and an Ag(s)|Ag(NO3)(aq) electrode (E° red = +0.80 V). Select the FALSE statement(s) concerning the operation of this cell: i) The concentration [Cu2+] decreases in the Cu half-cell. ii) The Ag electrode gains mass during operation of teh cell. iii) Cu metal is less easily oxidized than Ag metal. iv) The mass of the Cu electrode decreases during operation of the cell. v) Silver ions migrate from the Ag half-cell to the Cu half-cell through the salt bridge. i, iii, v ii, iv i, v ii, iii, iv all

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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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-.
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A 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.
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
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