6 Which of the following is/are true for an electrolytic cell for a system not at equilibrium (select ALL correct answers)?DA. AG is negative in the direction the reaction is proceedingOB. AG is positive in the direction the reaction is proceedingOC. AG is zeroOD.Ecell is negative in the direction the reaction is proceedingOE. Ecell is positive in the direction the reaction is proceedingOF. Ecell is zeroOG.Redox reaction is spontaneousOH. Redox reaction is not spontaneous01. Work can be done by the cellOJ. Work cannot be done by the cellA Moving to another question will save this response.:8:²80F3F9QF12WF2#3E$4aF4R%50F5TMacBook AirF66Y&7F7* 00DII8UF8

Answered: Image /qna-images/answer/20e9fa69-17ae-4ae1-844b-aaef112013de.jpg

Which of the following is/are true for an electrolytic cell for a system not at equilibrium (select ALL correct a DA. AG is negative in the direction the reaction is proceeding OB. AG is positive in the direction the reaction is proceeding OC. AG is zero OD.Ecell is negative in the direction the reaction is proceeding DE. Ecell is positive in the direction the reaction is proceeding OF. Ecell is zero OG.Redox reaction is spontaneous OH. Redox reaction is not spontaneous OI. Work can be done by the cell OJ. Work cannot be done by the cell A Moving to another question will save this response.

Which of the following is/are true for an electrolytic cell for a system not at equilibrium (select ALL correct a DA. AG is negative in the direction the reaction is proceeding OB. AG is positive in the direction the reaction is proceeding OC. AG is zero OD.Ecell is negative in the direction the reaction is proceeding DE. Ecell is positive in the direction the reaction is proceeding OF. Ecell is zero OG.Redox reaction is spontaneous OH. Redox reaction is not spontaneous OI. Work can be done by the cell OJ. Work cannot be done by the cell A Moving to another question will save this response.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter32: Voltaic Cell Measurements

Section: Chapter Questions

Problem 2ASA

See similar textbooks

Similar questions

Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
Use the following half-equations to write three spontaneous reactions. Justify your answers by calculating E° for the cells. 1. MnO4(aq)+8H+(aq)+5eMn2+(aq)+4H2OE=+1.512V 2. O2(g)+4H+(aq)+4e2H2OE=+1.229V 3. Co2+(aq)+2eCo(s)E=0.282V
For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a 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.
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)
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).
Consider a voltaic cell at 25°C in which the following reaction takes place: MnO2(s)+4H+(aq)+2Br(aq)Br2(l)+Mn2+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Find E under the following conditions: [Mn2+]=0.60M,[Br]=0.83M,pH=3.71 .
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
What is the voltage of a concentration cell of Cl ions where the concentrations are 1.045 and 0.085 M? What the spontaneous reaction?
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
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag