salt bridge 1.0 M (aq) 1.0 M (aq) Anode Cathode 1. A student constructs a voltaic cell to study the reaction between M(s) and X(s) and their ions. A diagram of the cell is shown above. The student uses 1.0 M solutions of M2* and X3+ as well as solid electrodes of M(s) and X(s). The reduction reactions of M2+ and X3+ are shown below. Reduction Standard Reduction Potential reaction (V) M2+ + 2 e- -0.35 M(s) X3+ + 3 e- X(s) +1.80 The student connects the voltaic cell and measures the voltage produced. a*. Write the net-ionic equation for the reaction that takes place in the voltaic cell b*.Determine the voltage produced by the cell ( C. A student states that the voltaic cell must be thermodynamically unfavorable since a voltage was produced. i. * Determine the value of AG° for the reactior ii. Do you agree or disagree with the student's slatement about thermodynamic favorability? Justify your answer by referring to AG° d. As the reaction proceeds would you expect the mass of the electrode used as the cathode to increase, decrease, or remain the same. Justify your answer. pte MacBook Pro

salt bridge 1.0 M (aq) 1.0 M (aq) Anode Cathode 1. A student constructs a voltaic cell to study the reaction between M(s) and X(s) and their ions. A diagram of the cell is shown above. The student uses 1.0 M solutions of M2* and X3+ as well as solid electrodes of M(s) and X(s). The reduction reactions of M2+ and X3+ are shown below. Reduction Standard Reduction Potential reaction (V) M2+ + 2 e- -0.35 M(s) X3+ + 3 e- X(s) +1.80 The student connects the voltaic cell and measures the voltage produced. a. Write the net-ionic equation for the reaction that takes place in the voltaic cell b.Determine the voltage produced by the cell ( C. A student states that the voltaic cell must be thermodynamically unfavorable since a voltage was produced. i. * Determine the value of AG° for the reactior ii. Do you agree or disagree with the student's slatement about thermodynamic favorability? Justify your answer by referring to AG° d. As the reaction proceeds would you expect the mass of the electrode used as the cathode to increase, decrease, or remain the same. Justify your answer. pte MacBook Pro

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 voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II) iodide solution is
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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?
(ii) State which species is the oxidising agent.
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)
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5. A more complex example where other atoms are involved. Balance the following reaction in basic solution. r (aq) + MnO4 (aq) MnO, (s)+ BrO;" (aq) TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E'(V) F + 20 H,0,(aq) + 2 H(aq)+2 e 2F(aq) 2.87 Stronger oxidizing agent Weaker 2 H,0 - PBSO (s) +2 H,0) -Mn0(s)+ 2 H,0) Mn (aq) 4 H,O) - Auts) 1.78 reducing agent PO,(s) + 4 H"(ag) + S0,2-(aq) + 2 e 1.69 Mno, (aq)+ 4 H'(aq) 3 e Mno, (aa) + 8 H (aq)+5 e Au (aq)+3e PbO,(s)+ 4 H(aa) + 2 e Cl,(g) + 2 e" 1.68 1.51 1.50 1.46 - P (ag) + 2 HO - 2a(aq) 1.36 1.33 Cr0, (aq) + 14 H'(ag) + 6 e 0+ 4 H (aq) + 4 e MnO(s)+4 H'(aq) +2 e 10, (aq) 6 H'(aq) + 5e Br+2e vo, (aq) + 2 H'(aq) + e NO, (aq) + 4 H°(aq) + 3e CIO+e 2 C"(aq) + 7 H,On - 2 H,O1) 1.23 Mn (aq) + 2 HyOV) 121 ulae) + 3 H,0() 2 Br (ag) - vo"(aq) +H,00 - NO + 2 H,O0 - CIO, (aa) - Agis) 1.20 1.09 1.00 0.96 0.95 Ag"(aa) + e 0.80 Fe (aq) + O+2 H'(aq)+2e - Fe*(aq) 0.77 - H,O,(ag) 0.70 Mn0, Taa) + e Mn0 (aa) 0.56 8) + 2 e…
(c) A galvanic cell is constructed using the following two half-cells at 25°C and 1 atm. The concentration of each species is given in the half-cell equation. Fe* (aq, 1.10 mol dm³) +3e → Fe2+ (aq, 0.86 mol dm³) E° = +0.77 V Ag* (aq, 1.35 mol dm³) + e → Ag(s) E° = +0.88 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)