A galvanic cell is powered by the following redox reaction:Br,(1) + H,(g) + 2 OH (aq)2 Br (aq) + 2 H,0(1)Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab.Write a balanced equation forthe half-reaction that takesplace at the cathode.Write a balanced equation forthe half-reaction that takesplace at the anode.Calculate the cell voltageunder standard conditions.ERound your answer to 2decimal places.ExplanationCheckO 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C80

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A galvanic cell is powered by the following redox reaction: Br,(1) + H,(g) + 2 OH (aq) 2 Br (aq) + 2 H,0(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. ロロ Write a balanced equation for the half-reaction that takes place at the cathode. ローロ Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places.

A galvanic cell is powered by the following redox reaction: Br,(1) + H,(g) + 2 OH (aq) 2 Br (aq) + 2 H,0(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. ロロ Write a balanced equation for the half-reaction that takes place at the cathode. ローロ Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

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Similar questions

A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.
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?
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.
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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.
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)

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