For the questions of Exp 20 Electrochemistry, Part A: Determination of the Faraday Constant Table 1: Data collected from the electrolysis apparatus in part A of the experiment that is needed to determine the faraday constant. Time=3098 sec current (i) = 0.101 A Volume of H2 collected = 43.02 mL Temperature of water = 26.0 celsius Pressure = 760 mmHg Answer the following questions with detailed calculations. a) Determine the faraday constant (C/mol). For the questions of Exp 20 Electrochemistry, Part B: EMF of Galvanic Cell Table 2: Electromotive force of the galvanic cell found through the mixtures of different solutions in part B of the experiment Experiment Solution A Electrode A Solution B Electrode B #4 Sn2+ Sn C42+ Cu #7 Zn2+ Zn 0.1 M KCI Ag Wire Answer the following question(s). a) Calculate E°cell for Experiment #4.

For the questions of Exp 20 Electrochemistry, Part A: Determination of the Faraday Constant Table 1: Data collected from the electrolysis apparatus in part A of the experiment that is needed to determine the faraday constant. Time=3098 sec current (i) = 0.101 A Volume of H2 collected = 43.02 mL Temperature of water = 26.0 celsius Pressure = 760 mmHg Answer the following questions with detailed calculations. a) Determine the faraday constant (C/mol). For the questions of Exp 20 Electrochemistry, Part B: EMF of Galvanic Cell Table 2: Electromotive force of the galvanic cell found through the mixtures of different solutions in part B of the experiment Experiment Solution A Electrode A Solution B Electrode B #4 Sn2+ Sn C42+ Cu #7 Zn2+ Zn 0.1 M KCI Ag Wire Answer the following question(s). a) Calculate E°cell for Experiment #4.

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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Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?
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Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
Calculate E°, G°, and K at 25°C for the reaction 3MnO4(aq)+4H+(aq)+Cl2(g)2Mn2+(aq)+2ClO3(aq)+2H2O
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 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=?
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