1. Draw the cell diagrams for each of the redox reactions given below. You may useplatinum as an inert electrode.a. 2 Al(s) + 3 H₂SO4(aq) → Al₂(SO4)3(aq) + 3 H₂(g)b. Fe₂(SO4)3 + 3 Pb(s) → 3 PbSO4(s) + 2 Fe(s)c. CuSO4(aq) + H₂(g) → Cu(s) + H₂SO4(aq)d. 2 NaBr(aq) + 12(g) → Br₂() +2 Nal(aq)e. 2 FeCl₂(aq) + SnCl₂(aq) → 2 FeCl3(aq) + Sn(s)f. 2 FeCl₂(aq) + SnCl(aq) → 2 FeCl3(aq) + SnCl₂(aq)See prob 18.1 for2. Consider a galvanic cell constructed from the following half-cells that are linked by aporous membrane. (1) an Au electrode dipped into 1.0 M Au(NO3)3 and (2) an Feelectrode dipped into 1.0 M FeSO4. Answer the following questions:a. Which electrode is the cathode?b. Write a balanced equation for the reaction occurring while the cell is discharging.c. What emf should the cell generate?Use Fig 18.1 ford. In what direction will electrons flow in the outer circuit?e. Toward which electrode will positive ions migrate?

As per the bartleby expert guidelines, I am allowed to answer first three parts of a question.…

. Draw the cell diagrams for each of the redox reactions given below. You may use platinum as an inert electrode. a. 2 Al(s) + 3 H₂SO4(aq) → Al2(SO4)3(aq) + 3 H₂(g) b. Fe₂(SO4)3 + 3 Pb(s) → 3 PbSO4(s) + 2 Fe(s) c. CuSO4(aq) + H₂(g) → Cu(s) + H₂SO4(aq) ON -Keg) Sen prob 181 f

. Draw the cell diagrams for each of the redox reactions given below. You may use platinum as an inert electrode. a. 2 Al(s) + 3 H₂SO4(aq) → Al2(SO4)3(aq) + 3 H₂(g) b. Fe₂(SO4)3 + 3 Pb(s) → 3 PbSO4(s) + 2 Fe(s) c. CuSO4(aq) + H₂(g) → Cu(s) + H₂SO4(aq) ON -Keg) Sen prob 181 f

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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Question

1. Draw the cell diagrams for each of the redox reactions given below. You may use
platinum as an inert electrode.
a. 2 Al(s) + 3 H₂SO4(aq) → Al₂(SO4)3(aq) + 3 H₂(g)
b. Fe₂(SO4)3 + 3 Pb(s) → 3 PbSO4(s) + 2 Fe(s)
c. CuSO4(aq) + H₂(g) → Cu(s) + H₂SO4(aq)
d. 2 NaBr(aq) + 12(g) → Br₂() +2 Nal(aq)
e. 2 FeCl₂(aq) + SnCl₂(aq) → 2 FeCl3(aq) + Sn(s)
f. 2 FeCl₂(aq) + SnCl(aq) → 2 FeCl3(aq) + SnCl₂(aq)
See prob 18.1 for
2. Consider a galvanic cell constructed from the following half-cells that are linked by a
porous membrane. (1) an Au electrode dipped into 1.0 M Au(NO3)3 and (2) an Fe
electrode dipped into 1.0 M FeSO4. Answer the following questions:
a. Which electrode is the cathode?
b. Write a balanced equation for the reaction occurring while the cell is discharging.
c. What emf should the cell generate?
Use Fig 18.1 for
d. In what direction will electrons flow in the outer circuit?
e. Toward which electrode will positive ions migrate?

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