STRYVISUALIZATION BatteriesZn(s) +2 OH (aq) Zn0(s) + H20(2) + 2e0:00URHgO(s) + H20(4)+2e Hg(e) + 20HT(aq)What is the overall reaction that occurs in the battery?CheckHext(6 of 6)Submit ncwor3 item attempts remainingcion

In this question, we will see the overall reaction occur in the given battery. You can see the…

Answered: Zn(s) +2 OH"(aq) Zn0(s) + H20(4) + 2e…

Zn(s) +2 OH"(aq) Zn0(s) + H20(4) + 2e 0:00 HgO(s) + H20(e) + 2e Hg(e) + 20HT(aq) e What is the overall reaction that occurs in the battery?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 39QAP: Use the following half-equations to write three spontaneous reactions. Justify your answers by...

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A solution containing a metal ion (M2+(aq)) is electrolyzed by a current of 7.8 A. After 15.5 minutes, 2.39 g of the metal is plated out. (a) How many coulombs are supplied by the battery? (b) What is the metal? (Assume 100% efficiency.)
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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
Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?
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Consider a cell reaction at 25°C where n=4 . Fill in the following table.
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