how.com/ilm/takeAssignment/takeCovalentActivity.do?locator=assignment-takeEMISTRY[References)Use the References to access important values if needed for this question.How many seconds are required to deposit 0.235 grams of copper metal from a solution that contains Cu*1ons, if a current of 1.16 A is applied.

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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 90AP: Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode...

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Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
Repeat the directions for Question 106 using a cell constructed of a strip of nickel immersed in a 1.0-M Ni2+ solution and a strip of silver dipping into a 1.0-M Ag+ solution. Write the balanced chemical equation for the reaction that is product-favored. Calculate the cell potential. Draw a sketch of the cell and indicate the anode, cathode, and direction of electron flow.
Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K
Calculate the equilibrium constant for the following reactions using data from the standard reduction potential tables. (a) Cl2(g)+2Br-(aq)Br2(g)+2Cl-(aq) (b) Ni(s)+2Ag+(aq)2Ag(s)+Ni2+(aq) (c) I2(s)+Sn2+(aq)2I(aq)+Sn4+(aq)
13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq)+4OH-(aq)N2(g)+4H2O(l)+4eO2(g)+2H2O(l)+4e4OH-(aq) (a) Which reaction occurs at the anode and which at the cathode? (b) What is the net cell reaction? (C) If the cell is to produce 0.50 A of current for 50.0 h, what mass in grams of hydrazine must be present? (d) What mass in grams of O2 must be available to react with the mass of N2H4 determined in part (c)?
Consult a table of standard reduction potentials and determine which of the following reactions are spontaneous under standard electrochemical conditions. (a) Mn(s)+2H+(aq)H2(g)+Mn2+(aq) (b) 2Al3+(aq)+3H2(g)2Al(s)+6H+(aq) (c) 2Cr(OH)3(s)+6F(aq)2Cr(s)+6OH(aq)+3F2(g) (d) Cl2(g)+2Br(aq)+Br2(l)+2Cl(aq)

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EMISTRY [References) Use the References to access important values if needed for this question. How many seconds are required to deposit 0.235 grams of copper metal from a solution that contains Cu* ions, if a current of 1.16 A is applied.