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 AG E A 1 - 124, kJ/mol 5.30 x 10 -1.28 V -99. kJ/mol 4.53 x 10 -1.03 V 1 -38. kJ/mol 2.20 x 10 0.39 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. calculated quantities (Check the box next to any that are wrong.) cell AG E A 1 - 124, kJ/mol 5.30 x 10 -1.28 V -99. kJ/mol 4.53 x 10 -1.03 V 1 -38. kJ/mol 2.20 x 10 0.39 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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Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) | Sn² + (0.0062 M). Sn +(0.15 M) || Fe +(0.11 M), Fe²+(0.0045 M) | Pt(s) ES' *Sn²+ = 0.154 V EF = 0.771 V Ecell 0.613 Incorrect Is the electrochemical cell spontaneous or not spontaneous as written at 25 "C? spontaneous not spontaneous
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
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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 1. calculated quantities (Check the box next to any that are wrong.) cell n AGº K A 1 -19. kJ/mol 4.69 × 10 0 E 0.20 V 13 B 1 77. kJ/mol 3.09 × 10 0.80 V -14 C 1 75. kJ/mol 7.25 X 10 0.78 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. 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
The chemical reaction that causes iron to corrode in air is given by: 4Fe+3O2→2Fe2O3 in which at 298 K, ΔHorxn = −1684 kJ and ΔSorxn = −543.7 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
The standard EMF for the cell using the overall cell reaction below is +0.84 V: 2Al(s) + 312 (s) 2A1³+ (aq) + 61 (aq) What is AGO for the cell reaction in kJ? Express your answer in decimal notation to one decimal place, without units.
Based on the sign of the standard cell potential, Eel, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Pb2*(aq) + H2(g) - Pb(s) + 2 H*(aq) Ni?*(aq) + s? (aq) Ni(s)+S(s) Al3+(aq) + 3 Na(s) → Al(s) + 3 Na*(aq)
Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = 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. me 1. ? • The cell potential under standard conditions E°. 00 2. His results are listed below. Ex 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. 000 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. 10 Ar cell n calculated quantities (Check the box next to any that are wrong.) K 0 E 27 A 2 156. kJ/mol O 2.14 X 10 0.81 V 11 B 2 66. kJ/mol O 3.65 × 10 -0.34 V C 2 -264. kJ/mol 46 1.78 x 10 -1.37 V K So Na G 4. 3.
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