plz help it dont do it confusing:The bottom part options are (from) or (to) The anode reaction is:A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge.Hg2+ (aq) + Ni(s). → Hg(l) + Ni²+(aq)+The cathode reaction is:+In the external circuit, electrons migrateUse the References to access important values if needed for this question.In the salt bridge, anions migrateEnter electrons as e.Use smallest possible integer coefficients for ALL reactions.If a box is not needed, leave it blank.++the Ni Ni2+ electrodethe Ni Ni2+ compartmentthe Hg | Hg2+ electrode.the Hg | Hg2+ compartment.

A voltaic cell generates electrical energy from chemical energy. It is driven by a spontaneous redox…

A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Hg2+ (aq) + Ni(s)→→→→→→Hg(1) + Ni²+ (aq) The anode reaction is: + The cathode reaction is: + In the external circuit, electrons migrate In the salt bridge, anions migrate + + the Ni Ni2+ electrode the Ni Ni²+ compartment the Hg| Hg2+ electrode. the Hg|Hg2+ compartment.

A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Hg2+ (aq) + Ni(s)→→→→→→Hg(1) + Ni²+ (aq) The anode reaction is: + The cathode reaction is: + In the external circuit, electrons migrate In the salt bridge, anions migrate + + the Ni Ni2+ electrode the Ni Ni²+ compartment the Hg| Hg2+ electrode. the Hg|Hg2+ compartment.

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 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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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?
The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O (in and solution) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the _______ electrode to the _____ electrode. Negative ions move in the salt bridge from the _____ half-cell to the ______ half-cell.
The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ______ electrode to the ____ electrode. Negative ions move in the salt bridge from the _____ half-cell to the _____ half-cell.
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.
Consider a cell reaction at 25°C where n=4 . Fill in the following table.
Consider a cell reaction at 25°C where n=2 . Fill in the following table.
A voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write equations for the oxidation and reduction half-reactions. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ______ half-cell to the ______ half-cell. The half-reaction at the anode is ____, and that at the cathode is _____.
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).