#78 78. Determine whether each redox reaction occurs spontane-ously in the forward direction.(a) Ca?+(b) 2 Ag*(aq) + Ni(s)(c) Fe(s) + Mn²*(aq)(d) 2 Al(s) + 3 Pb²*(aq)Ca(s) + Zn²*(aq):2+2 Ag(s) + Ni²*(aq)(aq) + Zn(s)Fe2+ (aq) + Mn(s)→ 2 Al* (aq) + 3 Pb(s)80. Suppose you wanted to cause Pb-+ ions to come out of so-du lution as solid Pb. What metal could you use to accomplishthis?82. Which metal in the activity series is oxidized with a Ni?+solution but not with a Cr*solution?84. Which metals dissolve in HCl? For those metals that dodissolve, write a balanced redox reaction showing whathappens when the metal dissolves.(a) Cr(b) РЬ(c) Au(d) Zn86. Make a sketch of an electrochemical cell with the overallreaction shown here. Label the anode, the cathode, and thesalt bridge. Indicate the direction of electron flow. Hint:When drawing electrochemical cells, the anode is usuallydrawn on the left side.

Answered: Image /qna-images/answer/ba5f7dd5-43da-4230-b3a8-7bbeac763a92.jpg

78. Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca?+ (aq) + Zn(s) (b) 2 Ag*(aq) + Ni(s) → 2 Ag(s) + Ni²*(aq) (c) Fe(s) + Mn²*(aq) (d) 2 Al(s) + 3 Pb²*(aq) Ca(s) + Zn²+(ag) Fe2+ (aq) + Mn(s) 2 Al*(ag) + 3 Pb(s)

78. Determine whether each redox reaction occurs spontane- ously in the forward direction. (a) Ca?+ (aq) + Zn(s) (b) 2 Ag(aq) + Ni(s) → 2 Ag(s) + Ni²(aq) (c) Fe(s) + Mn²(aq) (d) 2 Al(s) + 3 Pb²(aq) Ca(s) + Zn²+(ag) Fe2+ (aq) + Mn(s) 2 Al*(ag) + 3 Pb(s)

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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#78

78. Determine whether each redox reaction occurs spontane-
ously in the forward direction.
(a) Ca?+
(b) 2 Ag*(aq) + Ni(s)
(c) Fe(s) + Mn²*(aq)
(d) 2 Al(s) + 3 Pb²*(aq)
Ca(s) + Zn²*(aq)
:2+
2 Ag(s) + Ni²*(aq)
(aq) + Zn(s)
Fe2+ (aq) + Mn(s)
→ 2 Al* (aq) + 3 Pb(s)
80. Suppose you wanted to cause Pb-+ ions to come out of so-
du lution as solid Pb. What metal could you use to accomplish
this?
82. Which metal in the activity series is oxidized with a Ni?+
solution but not with a Cr*solution?
84. Which metals dissolve in HCl? For those metals that do
dissolve, write a balanced redox reaction showing what
happens when the metal dissolves.
(a) Cr
(b) РЬ
(c) Au
(d) Zn
86. Make a sketch of an electrochemical cell with the overall
reaction shown here. Label the anode, the cathode, and the
salt bridge. Indicate the direction of electron flow. Hint:
When drawing electrochemical cells, the anode is usually
drawn on the left side.

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