Use the information in the ALEKS Data tab to sort the following chemical species by reducing power. species reducing power Zn(s) choose one v Ag(s) choose one v Na(s) Mg(s) I choose one v choose one v X G

Use the information in the ALEKS Data tab to sort the following chemical species by reducing power. species reducing power Zn(s) choose one v Ag(s) choose one v Na(s) Mg(s) I choose one v choose one v X G

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 6CR: How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range...

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How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range corresponds to basic solutions? Why is pH = 7.00 considered neutral? When the pH of a solution changes by one unit, by what factor does the hydrogen ion concentration change in the solution? How is pOH defined? How arc pH and pOH for a given solution related? Explain.
Determine the standard free energy change, Gf, for the formation of S2-(aq) given that the Gf for. Ag*(aq) and Ag2S(s) are 77.1 kJ/mole and 395 kJ/mole respectively, and the solubility product for Ag2S(s) is 81051.
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?
The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, rG, for the reaction?
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.
• The standard reaction free energy AGº. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E°. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n AG K E 14 A 1 -81. kJ/mol 1.55 х 10 -0.84 V - 7 В 1 -38. kJ/mol 2.20 x 10 -0.39 V 14 C 1 81. kJ/mol 1.55 X 10 -0.84 V ?
7. Calculate the standard reduction potential and the standard free-energy change for each of the following coupled oxidation-reduction reactions. (a) Acetaldehyde + NADH + H E → Ethanol + NAD (b)UQH2 + 2 Cytochrome c (Fe") → UQ + 2 Cytochrome c (Fe2") + 2 H* (c) Succinate + ½ O2 → Fumarate + H2O
• The standard reaction free energy AG". • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell -19 4.03 x 10 A 105, k/molO 1.09 V 58. J/mol 30 1.45 x 10 -0.60 V C -94. KJ/mol 294 X 10 -0.97 V
8:51 AM Mon Dec 5 = S BIOL 286 E B Lecture Pow... Bb Lecture Pow... O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free... cell A B A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. C Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. n 1 AA 1 1 Explanation 142. kJ/mol O calculated quantities (Check the box next to any that are wrong.) AG - 50. kJ/mol O - 46. kJ/mol O Check www-awu.aleks.com K 24 7.54 x 10 O…
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. cell A B с n 2 2 2 calculated quantities (Check the box next to any that are wrong.) AGⓇ - 152. kJ/mol 81. kJ/mol -216. kJ/mol O K 26 4.26 X 10 1.55 X 10 6.94 X 10 14 37 X 0 E -0.79 V -0.42 V - 1.12 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG⁰. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. if any. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell A B C n 1 1 1 calculated quantities (Check the box next to any that are wrong.) AGº - 125. kJ/mol - 79. kJ/mol 57. kJ/mol K 1.26 X 10 6.92 × 10 9.68 × 10 - 22 13 0 E - 1.30 V 0.82 V -0.59 V
A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGO. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number ŉ of electrons transferred per redox reaction is 1. cell n A B U calculated quantities (Check the box next to any that are wrong.) AGⓇ 139. kJ/mol O 65. kJ/mol -98. kJ/mol K 24 2.25 × 10 4.10 × 10 6.78 × 10 - 12 18 0 E - 1.44 V 0.67 V 1.02 V