A student made measurements on some electrochemical cells and calculated three quantities:The standard reaction free energyAGº.• The equilibrium constant K at 25.0 °C.• The cell potential under standard conditions E".His results are listed below.oloUnfortunately, 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.ArNote: 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.)cellnaGKE- 517.85 X 10A2286. kJ/mol1.48 V26В2154. kJ/mol9.54 X 100.80 V10C- 60. kJ/mol3.25 X 10-0.31 V

Here we required to find the error in the Gibbs free energy,equilibrium constant and standard cell…

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 AG K E A 286. kJ/mol O -51 7.85 x 10 1.48 V 26 9.54 x 10 B 2 154. kJ/mol 0.80 V 10 C 2 - 60. kJ/mol 3.25 x 10 -0.31 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 AG K E A 286. kJ/mol O -51 7.85 x 10 1.48 V 26 9.54 x 10 B 2 154. kJ/mol 0.80 V 10 C 2 - 60. kJ/mol 3.25 x 10 -0.31 V

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. calculated quantities (Check the box next to any that are wrong.) cell n aG° E K 11 8.19 × 10 А 2 68. kJ/ mol O 0.35 V В 2 - 114. kJ/mol 20 1.07 x 10 0.59 V C 2 42. kJ/mol 7 2.28 X 10 - 0.22 V
• 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 rom 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 correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. cell A B C Explanation n 1 1 1 calculated quantities (Check the box next to any that are wrong.) 0 AG 37. kJ/mol O Check 90. kJ/mol -143. kJ/mol O 6 3.03 × 10 5.85 x 10 hical cells and calculated three quantities: 1.13 X 10 15 25 O X 0 E 0.38 V -0.93 V -1.48 V O O MacBook Air Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of
• The siandard 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 AG K E 4 А 1 26. kJ/mol O 3.59 x 10 0.27 V 23 В 1 134. kJ/mol 2.99 X 10 -1.39 V C 1 -41. kJ/mol 1.52 X 10 -0.42 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 E K 39 A 226. kJ/mol O 3.92 x 10 1.17 V 21 В 2 120. kJ/mol 1.05 X 10 -0.62 V 2 - 214. kJ/mol 37 3.10 X 10 - 1.11 V ?
A student made measurements on some electrochemical cells and calculated three quantities: The standard reaction free energy . The equilibrium constant at . The cell potential under standard conditions . 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 of electrons transferred per redox reaction is .
A student made measurements on some electrochemical cells and calculated three quantities: AG. • The equilibrium constant K at 25.0 °C. • The standard reaction free energy • The cell potential under standard conditions 圖 His results are listed below. dlo 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 AG K E 8- A -41. kJ/mol 6.56 x 10 -0.42 V 15 8.76 x 10 1 -91. kJ/mol - 0.94 V 17 1.52 x 10 1 -96. kJ/mol - 1.00 V Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility MAY 8. MacBoo 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 E". 圖 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. do 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 AG° E K A 2 268. kJ/mol O 46 8.95 x 10 -1.39 V -38 B -212. kJ/mol 7.23 x 10 1.10 V 27 2.14 x 10 2 -156. kJ/mol O -0.81 V Explanation Check Privacy Accessibility 02021 McGraw-Hill Education. All Rights Reserved. Terms of Use MacBook Air F12 ►► FI F10 F9 F7…
The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2 H2O(I) + 2 NO2(g). Thestandard cell potential at 25 °C is -0.04 V. Calculate the electricalwork that can be done by the cell.
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 2. calculated quantities (Check the box next to any that are wrong.) cell n AGⓇ ΔG K Eº - 32 A 2 А -178. kJ/mol 6.54 × 10 -0.92 V B 179. kJ/mol 2.29 X 10 -0.93 V с 2 127. kJ/mol 1.78 × 10²2 0.66 V 31 X ?
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 AG K E A 181. kJ/mol 5.13 x 10 -0.94 V 162. kJ/mol 2.41 x 10 0.84 V 66. kJ/mol 3.65 x 10 0.34 V Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Ac MAY 8. 2. 2. 2.
The free energy change for the following reaction at 25 °C, when Sn²+ 2+ [Zn²+] = 0.00776 M, is -133 kJ: [Sn²+] = 1.11 M and Sn²+ (1.11 M) + Zn(s) → Sn(s) + Zn²+ AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Ecell V Sn(s) + Zn²+ (0.00776 M) Would this reaction be spontaneous in the forward or the reverse direction? O forward direction O reverse direction
The Nernst equation can be used to calculate... A. cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard B. standard cell potentials from standard reduction potentials C. cell potentials given only the temperature and reactant concentrations D. cell potentials from standard oxidation potentials E. the change in standard Gibbs free energy from standard cell potentials