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 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.) AGⓇ 98. kJ/mol O -131. kJ/mol -145. kJ/mol O O K 17 1.48 × 10 O 1.12 x 10 -23 25 2.53 x 10 O O X 0 E -1.02 V -1.36 V -1.50 V 5 O O O

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 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.) AGⓇ 98. kJ/mol O -131. kJ/mol -145. kJ/mol O O K 17 1.48 × 10 O 1.12 x 10 -23 25 2.53 x 10 O O X 0 E -1.02 V -1.36 V -1.50 V 5 O O O

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 ...
Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣ Au3+(aq,? M) ∣ Au (s)Determine the standard cell potential and if the cell is more spontaneous or less spontaneous at standard conditions.
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
Calculate the K and AG for the following reaction at 25 °C: с Zn(s) + CuSO₂ (aq) = ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °℃ and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. K с Part 2 of 2 = AGO = x10 Round your answer to 4 significant digits. kJ mol X Ś x10
A concentration cell is one wherein the concentrations of the same ion in the two electrodes are different. Due to this difference, a potential is measured but there is no redox reaction taking place. Consider the following data for a concentration cell consisting of copper ions. The cell notation is given as Cu| Cu2+ (x M) || Cu2+ (y M) | Cu Verify the accuracy of the cell potentials measured at 27.5°C shown in the table below for a copper concentration cell using the Nernst Equation. Show your complete solution to justify your conclusion. [Cu2*], [Cu2*], cathode Ecell anode 0.0310 0.01 0.10 0.0347 0.01 0.15 0.0382 0.01 0.20 0.0421 0.01 0.25 0.0450 0.01 0.30
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