A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(9)+4 H,O(1)+4e - N,H4(aq)+4 OH (aq) =-1.16 V Pred 2+ Zn“"(aq)+2e • Zn(s) :-0.763 V 'red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Oxto Write a balanced equation for the half-reaction that happens at the anode. ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(9)+4 H,O(1)+4e - N,H4(aq)+4 OH (aq) =-1.16 V Pred 2+ Zn“"(aq)+2e • Zn(s) :-0.763 V 'red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Oxto Write a balanced equation for the half-reaction that happens at the anode. ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

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...

See similar textbooks

Similar questions

Given the following data, answer the following questions: Fe2+(aq) + 2e- → Fe(s) E○red = -0.44 v, Cr3+(aq) + e- → Cr2+(aq) E○red = -0.407 v (a) What is the spontaneous cell reaction when a voltaic cell is constructed using these two half- reactions? (b) What is the E○ for the reaction?(c) What is equilibrium constant and deltaG?(d) If the concentration of Cr3+ and Cr2+ are each 0.10 M and the cell potential is 0.100 v, what is the concentration of Fe2+?(e) What is E for the reaction at equilibrium?
What is the net reaction for the cell? Is it .44V or .22V?
MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation:
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)
Consider the half reactions in a cell: Pb2+ + 2 e ------ Pb(s) Eo = - 0.126 V Fe3+ + e ------ Fe2+ (aq) Eo = + 0.771 V Which of the following statement is correct for the cell? Given Given A. For a Galvanic cell the standard emf will be 0.645 V and Pb will be the anode B. For a Galvanic cell standard emf will be 0.645 V and Fe will be the cathode C. For a Galvanic cell standard emf will be 1.668 V and Pb will be cathode D. For a Voltaic cell the standard emf will be 0.897 V and Fe will be the anode E. For a Voltaic cell standard emf will be 0.897 V and Pb will be the anode