a) Consider the sparingly soluble salt lead(II) sulfate. Write a balanced chemical equation showing the dissolution of lead(II) sulfate. b) Given the following information, provide the net reaction for the spontaneous reaction and determine the cell potential under standard conditions that would occur from these two half-reactions: Pb2"(aq) + 2e- → Pb(s) E°red = -0.1262 V PbSO4(s) + 2e- → Pb(s) + SO4² (aq) E°red = –0.3505 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b.

a) Consider the sparingly soluble salt lead(II) sulfate. Write a balanced chemical equation showing the dissolution of lead(II) sulfate. b) Given the following information, provide the net reaction for the spontaneous reaction and determine the cell potential under standard conditions that would occur from these two half-reactions: Pb2"(aq) + 2e- → Pb(s) E°red = -0.1262 V PbSO4(s) + 2e- → Pb(s) + SO4² (aq) E°red = –0.3505 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b.

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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When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic cell in which solid lead(II) sulfate (PbSO4) is reduced to lead at the cathode and oxidized to solid lead(II) oxide (PbO) at the anode. Suppose a current of 80.0 A is fed into a car battery for 63.0 seconds. Calculate the mass of lead deposited on the cathode of the battery. Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol. x10 0.0 X μ 010 3
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A galvanic cell is powered by the following redox reaction: 3+ 4 Fe (aq) + N,H,(aq) + 4 OH (aq) 2+ 4 Fe" (aq) + N,(g) + 4H,O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = v %3D Round your answer to 2 decimal places. Explanation Check © 2021 McGraw-Hill Education, All Rights Reserved. P Type here to search
4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.
(ii) State which species is the oxidising agent.
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.
(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
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Use the tabulated half-cell potentials to calculate ΔG° for the following reaction. (Hint: Before you being, you must determine whether or not the reaction is balanced.)I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq) (a)‒1.1×102kJ (b) +4.9×101kJ (c) ‒9.7×101kJ (d) ‒3.3×102kJ