2. Use standard reduction table on page 1 to help you answer this question. Cu Metal M Salt bridge 1.0 M M(NO,), 1.0 M Cuso, When the voltaic cell above is hooked up, the voltmeter reads +2.00 V and the mass of the metal electrode M decreases. a. Is electrode “M" the anode or the cathode. Justify your answer. b. Calculate the standard half-cell reduction potential E°red for the electrode “M". c. Identify the solid metal and the metal cation that react at electrode “M". Write the electron configuration for the cation. d. Write the balanced net ionic equation for the overall reaction that takes place in this voltaic cell. e. Describe the direction of electron flow in this cell (quick sketch on your paper or in words). f. If the concentration of metal M were increased, predict what would happen to the cell potential (increase, decrease or stay the same). Justify your answer.

2. Use standard reduction table on page 1 to help you answer this question. Cu Metal M Salt bridge 1.0 M M(NO,), 1.0 M Cuso, When the voltaic cell above is hooked up, the voltmeter reads +2.00 V and the mass of the metal electrode M decreases. a. Is electrode “M" the anode or the cathode. Justify your answer. b. Calculate the standard half-cell reduction potential E°red for the electrode “M". c. Identify the solid metal and the metal cation that react at electrode “M". Write the electron configuration for the cation. d. Write the balanced net ionic equation for the overall reaction that takes place in this voltaic cell. e. Describe the direction of electron flow in this cell (quick sketch on your paper or in words). f. If the concentration of metal M were increased, predict what would happen to the cell potential (increase, decrease or stay the same). Justify your answer.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 160MP

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Similar questions

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?
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
Suppose Ered for H+H2 were taken to be 0.300 V instead of 0.000 V. What would be (a) Eox for H2H+ ? (b) Ered for Br2Br ? (c) E for the cell in 34(c)? Compare your answer with that obtained in 34(c).
Consider 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?
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-.
Consider the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)