c) Explain why significant deviations are often observed from the behaviour anticipated from phase diagrams. In particular consider what happens when cooling from the liquid to the solid state. d) Calculate the AG° in kJ/mol for a Mg battery with a theoretical standard potential of 3.11 V. e) In secondary batteries, replacing i) Li* with Na+ cations and ii) liquid electrolytes with solid electrolytes are both topical research subjects. Indicate a benefit and a challenge for each of these approaches.

c) Explain why significant deviations are often observed from the behaviour anticipated from phase diagrams. In particular consider what happens when cooling from the liquid to the solid state. d) Calculate the AG° in kJ/mol for a Mg battery with a theoretical standard potential of 3.11 V. e) In secondary batteries, replacing i) Li* with Na+ cations and ii) liquid electrolytes with solid electrolytes are both topical research subjects. Indicate a benefit and a challenge for each of these approaches.

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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THE QUESTION Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination will give maximum potential. Provide justification. THE DATA GIVEN IN QUESTION 4 IS HERE (c) Arrange the following electrodes in ascending order of reducing capacity. And provide suitable explanation. Zn2* (aq) + 2e Zn(s): E° = -0.76 V %3D Ag*(aq) + e –→ Ag(s): E° = 0.8 V Ca2+ (aq) + 2e Ca(s): E° = -2.87 V Cu2* (aq) + 2e→ Cu(s): E° = 0.34 V
10.)
a) Consider the sparingly soluble salt silver bromide. Write a balanced chemical equation showing the dissolution of silver bromide. 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: Ag+(aq) + e- ⟶⟶ Ag(s) E°red = 0.80 V AgBr(s) + e- ⟶⟶ Ag(s) + Br-(aq) E°red = 0.07 V c) Calculate the equilibrium constant at 283 K (10.° C) for the spontaneous redox reaction you wrote in part b. d) Using only the information provided in this problem, calculate the solubility product constant of silver bromide at 10. °C. e) Is the dissolution of silver bromide at 10. °C thermodynamically favorable? Justify your response by determining ΔΔG°rxn at 10. °C, using only the information provided or determined in this problem.
Caculate ℰ° values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
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)
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ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.99 minutes for a current of 1.36 A to plate 0.0603 g of metal from a solution containing M2(SO4)3- (Round off the final answer to TWwo decimal places. Do not include the unit.)
Calculate the potential of the cell when; [I] = 0.75 M, pH = 8.90, T= 300 K, P(H2) = 60 torr. Of course (R = 8.314 J/mol.K) and (F = 96500 J/V.mol).
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2+ half-cell and an H2/H+ half-cell under the following conditions: [Zn2+ ] = 0.041 M [H+ ]= 1.2 M partial pressure of H2 = 0.52 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2+ (aq) + 2e Zn(s) E° = 0.76 V 2H+ (aq) + 2e H2(g) E° = 0.00 V
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