M1xUse the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energychange in kJ for the reaction:F2Answer:#3ED2+Co²+ (aq) + Sn(s) → Co(s) + Sn²+ (aq)K for this reaction would beSubmit AnswerCF3$4RF[Review Topics][References]Use the References to access important values if needed for this question.(1)F4VKJRetry Entire Group%5TDIIGCengage Learning Cengage Technical SupportF5A6-0than one.Y8 more group attempts remainingHF6&7B N-*UF7J*PrtScn8MF8KHome9F9OLLEnd0F10P>PreviousPgUpF11{[?NextSave and ExitPgDn+119:55 PM12/2/2022F12InsDelBackspa1

Given that, a redox reaction is Co2+(aq) + Sn(s) → Co(s) + Sn2+(aq). We have to calculate the…

se the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy mange in kJ for the reaction: 2+ Co²+ (aq) + Sn(s)→ Co(s) + Sn²+ (aq) Answer: kJ K for this reaction would be Submit Answer Retry Entire Group than one. 8 more group attempts remaining

se the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy mange in kJ for the reaction: 2+ Co²+ (aq) + Sn(s)→ Co(s) + Sn²+ (aq) Answer: kJ K for this reaction would be Submit Answer Retry Entire Group than one. 8 more group attempts remaining

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...

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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)?
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
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)
Consider the following cell reaction at 25C. 2Cr(s)+3Fe2+(aq)2Cr3+(aq)+3Fe(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain G for the cell reaction. Use data in Appendix C to calculate H; note that Cr(H2O)63+(aq) equals Cr3+(aq). Use these values of H and G to obtain S for the cell reaction.
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mg(s)+Ni2+(aq)Mg2+(aq)+Ni(s) (b) 2Ag+(aq)+Cu(s)Cu2+(aq)+2Ag(s) (c) Mn(s)+Sn(NO3)2(aq)Mn(NO3)2(aq)+Sn(s) (d) 3Fe(NO3)2(aq)+Au(NO3)3(aq)3Fe(NO3)3(aq)+Au(s)
The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard conditions. Write out the Nernst equation. What are nonstandard conditions? What do , n, and Q stand for in the Nernst equation? What does the Nernst equation reduce to when a redox reaction is at equilibrium? What are the signs of G and when K 1? When K 1? When K = 1? Explain the following statement: determines spontaneity, while determines the equilibrium position. Under what conditions can you use to predict spontaneity?
Consider the following galvanic cell at 25C: Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|Co The overall reaction and equilibrium constant value are 2Cr2+(aq)+Co2+(aq)2Cr3+(aq)+Co(s)K=2.79107 Calculate the cell potential, for this galvanic cell and G for the cell reaction at these conditions.
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?