yan ecersiz sayılacaktirl. 1. 1) If a cell generates current by itself, that is, if it operates as a battery, the electrode marked (-) is the anode. 1) EIf an electric current is applied from outside, the electrode marked (-) is the anode. I) The electrode with a large oxidation potential in a Galvanic cell is marked (-). IV) In order for the battery to generate current by itself, the potential of the battery (Epil) must be positive. Which of the above is/are wrong. I ve III A-) Il ve I B-) I ve V C-) Yalnz i D-) Yalnz IV E-)

yan ecersiz sayılacaktirl. 1. 1) If a cell generates current by itself, that is, if it operates as a battery, the electrode marked (-) is the anode. 1) EIf an electric current is applied from outside, the electrode marked (-) is the anode. I) The electrode with a large oxidation potential in a Galvanic cell is marked (-). IV) In order for the battery to generate current by itself, the potential of the battery (Epil) must be positive. Which of the above is/are wrong. I ve III A-) Il ve I B-) I ve V C-) Yalnz i D-) Yalnz IV E-)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.3QAP

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Similar questions

Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
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).
If a 2.5 A current is run through a circuit for 35 minutes, how many coulombs of charge moved through the circuit?
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?
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)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
An active (metal) electrode was found to gain mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
The following two half-reactions arc involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag++eAgE=0.80VNi2++2eNiE=0.25V
For the standard cell potentials given here, determine the ?G for the cell in k].. (a) 0.000V,n=2 (b) +0.434V,n=2 (c) -2.439 V, n = 1
Based on the cell potential measured for the cells Co(s)|Co2+(aq) Cu 2+( aq)|Cu( s)E=0.614VFe(s)|Fe2+(aq) Cu 2+( aq)|Cu( s)E=0.777V what potential should you expect to find for the following cell? Fe(s)|Fe2+(aq)Co2+(aq)|Co(s)
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.

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