Fill in the BlanksType your answers in all of the blanks and submitUsing the standard reduction potentials from Appendix 11 determine the cell potential, &, for this redox reaction then fill in thecell-blanks for this question.10 (s) + 2 Fe(OH)2(5) + H20()I (aq) 2 Fe(OH)3(5)The , for this reaction iscellType your answer hereXV.You are incorrectThe AG for this reaction isType your answer here XkJ/mole.You are incorrectAs written this reaction isspontaneous(Enter spontaneous or nonspontaneous)You are correct

In the given Redox reaction reduction and oxidation half is: Cathode(reduction): IO- + H2O + 2e-…

Fill in the Blanks Type your answers in all of the blanks and submit Using the standard reduction potentials from Appendix 11 determine the cell potential, Eell, for this redox reaction then fill in the blanks for this question. 10 (s) +2 Fe(OH)2(s) + H20(D→I (aq) + 2 Fe(OH)3 (5) The Ecell V. for this reaction is Type your answer here You are incorrect The AG for this reaction is Type your answer here kJ/mole. You are incorrect As written this reaction is (Enter spontaneous or nonspontaneous.) spontaneous You are correct

Fill in the Blanks Type your answers in all of the blanks and submit Using the standard reduction potentials from Appendix 11 determine the cell potential, Eell, for this redox reaction then fill in the blanks for this question. 10 (s) +2 Fe(OH)2(s) + H20(D→I (aq) + 2 Fe(OH)3 (5) The Ecell V. for this reaction is Type your answer here You are incorrect The AG for this reaction is Type your answer here kJ/mole. You are incorrect As written this reaction is (Enter spontaneous or nonspontaneous.) spontaneous You are correct

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

Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
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).
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
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)
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
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)?