NO.:DATE:An electro chemicalis vet upelectrodecellwithco pperCu s04 lag) and1.0mol L tb (NOs)z cag).inContactwith1.0 mol La leaddcctrodewithincontactthe utandard reduction potentials arPbt t 2c-E° -0 13V2+E° +0-34Vthir galuanicincelAt25°Cthe standcrdcell potential Forvo Hs

A numerical problem based on electrochemistry, which is to be accomplished.

Answered: An electro chemi cal cell is set up…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Standard Reduction Potentials at Standard States and 25°C Pb(s) + 2H1+(0.0010 M) Pb2*(.50 M) + H2(1.2 atm) Half-reaction EV) 2H 20) + 2e → Hxa Pb ag) 0.0 -0.13 +2e Pb(O (a) Calculate the cell emf for the above reaction at 25°C. (b) Are reactants or products favored at equilibrium? Explain your answer. (c) In which direction will the reaction proceed to reach equilibrium? Explain your answer.
22. Given the electrochemical reaction shown, if the standard reduction potential of Zn2* > Zn is -0.76V, what is the standard reduction potential of Mg2+ → Mg? Mg / Mg 2"(ag) // Zn (ag) / Zn C. +2.37 V E = +1.61 V e. none of the above a. -0.85 V b. +0.85 V d. -2.37 V
A galvanic cell consists of a Fe electrode in a 1.0 M FeSO4 solution and a Ni electrode in a 1.0 M NiSO4 solution. Calculate the Eocell at 25°C. -0.19V 0.19V -0.69V 0.69V
(b) Use the listing of standard reduction potentials on page 10 to determine the E° for Ce**(aq) + 4e → Ce(s) Reduction half-reaction E/V Reduction half-reaction E/V Ag Ag Age Ag Agir + Ag+ Br AgCleAg+a 1+ 2e21 15+2e3r In'+eIn In+e In In + 2e In In"+ SeIn In" In K*+ K La+ ela Li Mg+ 2- Mg Mn"+ 2e Mn Mn+e Mn MnO, + 4+ 2e- Ma + 2H,o MnO; + SH + Se Mn+ 4H,0 MnO; +eMno}- Mno + 21,0+ 2eMno, + 4OH Na' +e Na NP+ 2e NI NIOOH + H,0+ Ni(OH), +OH NO;+2H+e NO, + H,0 NO; + H+ - NO+ 2H,0 NO; + H,0+ 2e- NO; + 20H O,+2H,0+ de-→ 4OH 0,+ 4H+ de 2H,0 40.80 +0.54 +1.98 +0.53 +0.0713 -0.14 +0.22 -0.40 AgCro, + 2e 2Ag+ Cro AgF+e Ag +F Agl + Ag+ r Al+ Se Al +0.45 -0.44 +0.78 -0.34 -0.15 -0.49 -1.66 -2.93 Au' +eAu Au+ Se Au Ba+ 2e-Ba Be+ 2eBe +1.69 -2.52 +1.40 -3.05 +2.91 -2.36 -L8S -1.18 +0.20 +1.51 Br, + 2e 2Br Bro +H,0+ 2e Br+ 20H Cal+ 2eCa Ca(OH), + 2e Cd+ 20H Ca + 2eCd Ce+ Ce +1.09 +1.23 +0.76 +1.51 -2.87 +0.56 -0.81 +0.60 -0.40 -2.71 -2.48 -0.23 CeteCe" +1.61 +0.49 a,+ 2e-2 CIO +H,0+ 2→a+20H CO;+ 2H+ 2e…
What is the standard cell voltage at 25.0oC for the reaction below?Hg2+(aq) + 2MnO42-(aq) ↔ Hg(l) + 2MnO4-(aq) K = 6.44e9 -0.290 V 0.290 V 0.126 V -0.126 V
iles Tab Window Help Wed A V Prc V We V Sli V Si V Si V ES x b Se G WI C A) C 1)A E Es G Us keCovalentActivity.do?locator=assignment-take [Review Topics] [References] Use the References to access important values if needed for this question. What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg+ concentration is 4.94 × 10¬ª M and the Alº* concentration is 1.16 M ? 3H3²+ (aq) + 2Al(s) → 3Hg(1) + 2AI³+ (aq) Ecell =|| V The cell reaction as written above is for the concentrations given. Submit Answer Retry Entire Group 2 more group attempts remaining Next Previous Show All MacBook Pro * & $ 8 9 6 7 4 { [ P Y E R %3D K
Use the standard reduction potentials given below to predict if a reaction will occur when Sn metal is put into a 1 M aqueous Mg2+ solution. Sn2+(aq)+ 2e- ---> Sn(s) E°red = -0.140V Mg2+(aq) + 2e- ---> Mg(s) E°red = -2.370V If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) _______ +_______ ------>_______ + ________
4. Calculate the standard reduction potential of the half-cell electrode below if the standard reduction potential for Au3+ is E° = 1.52V and the formation constant of the AuBr4- is Kf = 1.169e+34 AuBr4- (aq) + 3e- --> Au(s) + 4Br-
gine.html?ClassID=1563099459# e.. How many seconds will it take to reduce 2.2 g Au from an aqueous Au3+ solution at a current of 7.5 A? Au3+ + 3e -→ Au Ered = 1.51 V t = [?] sec Time (sec) Enter
What is the standard electrode potential for the reaction 2 Cr + 3 Pb2* →3 Pb + 2 Cr+? Standard Reduction E° (V) V Potentials Pb2+(aq) + 2e Pb(s) -0.13 1 4 6. Cr3+(aq) + 3e- - Cr(s) -0.74 8. 6. +/- 0. 2. 7.
Im using this formula: E = Ecell - 0.0257/n (ln) (Q)

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