3. Calculate the standard cell potential for the following reaction and determine whether the reaction is spontaneous or nonspontaneous as written. Mg(s) + Cl2(g) Mg²* + 2Cl (aq) Mg* + 2e 5 Mg(s) E°=1.360 V Cl2 + 2e 5 2Cl A. 1.628 V, spontaneous E° = 0.268 V B. -1.628 V nonspontaneous C. 1.094 V, spontaneous D. -1.094 V , nonspontaneous E. None of the answers

3. Calculate the standard cell potential for the following reaction and determine whether the reaction is spontaneous or nonspontaneous as written. Mg(s) + Cl2(g) Mg²* + 2Cl (aq) Mg* + 2e 5 Mg(s) E°=1.360 V Cl2 + 2e 5 2Cl A. 1.628 V, spontaneous E° = 0.268 V B. -1.628 V nonspontaneous C. 1.094 V, spontaneous D. -1.094 V , nonspontaneous E. None of the answers

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 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
What is E at 25 °C for the reaction described by Mg(s) | Mg²⁺ (1.60 M) || Pb²⁺ (0.850 M) | Pb(s)? The standard cell potential for the reaction is +2.231 V.
The free energy change for the following reaction at 25 °C, when [H*] = 1.11 M and [Sn2+] = 1.21x10-3 M, is -43.9 %3D kJ: 2H*(1.11 M) + Sn(s) H2(g) + Sn2+(1.21x10-3 M) AG = -43.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction v forward reverse
Calculate the K and AG for the following reaction at 25 °C: Mg(s) + Pb2+(aq)=Mg2+(aq) + Pb (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Кс Part 2 of 2 G Round your answer to 4 significant digits. AG° kJ mol
Given the following two half-reactions, determine which overall reaction is spontaneous, and calculate its standard cell potential. Cd2*(aq) + 2 e- Cd(s); E° = -0.403 V Zn2"(aq) + 2 e-Zn(s); E° = -0.763 V O A. Cd(s) + Zn2*(aq) OB. Cd(s) + Zn(s)¯ OC. ca²*(aq) + Zn²*(aq)' Cd2+(aq) + Zn(s); E° = -0.360 V Cd2*(aq) + Zn²+(aq); E° = -1.166 V PCd(s) + Zn(s); E° = +1.166 V O D. Cd2+(aq) + Zn(s) cd(s) + Zn2*(aq); E° = +0.360 V
The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M) ΔG = 68.1 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
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
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
10. What is the standard cell potential of the following electrochemical cell at 25°C: Ni(s) I NiCl2(aq) || Cu(NO3)2 (aq) | Cu(s) a. 0.62 V b. -0.62 V с. 0.60 V d. -0.60 V e. 0.095 V enstant fr ther
The standard state cell potential for the reaction below is 1.030 V. Zn(s) + Hg,Cl,(s)→ ZnCl,(aq) + 2Hg(1) Calculate the standard state Gibb's energy change (in kJ) at 298K for the reaction. O -99.4 kJ O -199 kJ O 199kJ O 99.4 kJ
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