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 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 iscorrect.Also note: for each cell, the number n of electrons transferred per redox reaction is 2.calculated quantities(Check the box next to any that are wrong.)cellAGKE-8A2-41. kJ/mol6.56 x 10-0.21 V501.27 x 10B2- 286. kJ/mol-1.48 V-152-81. kJ/mol6.45 x 10-0.42 V

For an electrochemical cell, the relationship between change in standard gibbs free energy and…

Answered: A student made measurements on some…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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 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 2. cell n A B C 2 2. 2 calculated quantities. (Check the box next to any that are wrong.) .0 AG 172. kJ/mol J 127. kJ/mol - 170. kJ/mol K -31 7.36 X 10 5:63 X.10 - 23 29 6.06 × 10 - O O E -0.89 V. 0:66 V -0.88. V 5
Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation: M| M+||N3+|N with reduction potential of 0.36 V for M and 1.05 V for N, respectively. (Note that M and N are fake metals). Calculate the value of ∆G° in J. F = 96500 C/mol e- Enter your answer in scientific notation with 2 decimal places and be sure to include the correct sign. Example: -2.34e+6 or 1.23e-5. Note e is used for "x10" in this notation! Do NOT type "x 10"!
Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.5M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.19 volts. Your Answer:
Give a clear explanation handwritten answer ...
The standard voltage, Eº, for the reaction of Zn(s) and Cl₂(g) is 2.12 V. What is the standard Gibbs free energy change, AGO, for the reaction? J/mol
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the cell potential (Ecell), in volts, for this reaction at 35.4 °C when [M+] = 0.00533 M and [N2+] = 0.725 M? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) E°cell = 0.128 V
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 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 2. calculated quantities (Check the box next to any that are wrong.) cell n AG K E - 16 1.14 X 10 A 2 -91. kJ/mol -0.47 V - 49 1.98 x 10 B 2 - 278. kJ/mol 1.44 V - 44 5.34 x 10 2 247. kJ/mol 1.28 V
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 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. cell A B C₁ n 1 1. 1 calculated quantities (Check the box next to any that are wrong.) ·a AG 77. kJ/mol O 64. kJ/mol 35. kJ/mol O O K 3.09 X 10 6:13 X 10 13. 6 1.35 X 10 - 12. O X 0. 0.80 V 0.66 V -0.36 V Ś
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 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 46° K 1 - 124. kJ/mol 5.30 x 10 21 -1.28 V -18 4.53 x 10 B 1 - 99. kJ/mol -1.03 V -7 2.20 x 10 1 - 38. kJ/mol 0.39 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 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 -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V
The standard cell potential is a thermodynamic state func-tion. How are E° values treated similarly to ΔH°, ΔG°, and S°values? How are they treated differently?
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. 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, if 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 n A B C 1 calculated quantities (Check the box next to any that are wrong.) AGⓇ 37. kJ/mol - 66. kJ/mol -47. kJ/mol K 6 3.03 × 10 2.74 × 10 5.83 × 10 12 9 X 0 E -0.38 V 0.68 V -0.49 V S

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