18.16 Predict whether the following reactions would occur spontaneously in aqueous solution at 25°C. Assume that the initial concentrations of dissolved species are all 1.0 M. (a) Ca(s) + Cď²* (aq) → Ca?* (aq) + Cd(s) (b) 2B1¯(aq) + Sn²*(aq) (c) 2Ag(s) + Ni²* (aq) (d) Cu*(aq) + Fe** (aq) Br;(1) + Sn(s) 2Ag*(aq) + Ni(s) Cu²* (aq) + Fe²* (aq)

18.16 Predict whether the following reactions would occur spontaneously in aqueous solution at 25°C. Assume that the initial concentrations of dissolved species are all 1.0 M. (a) Ca(s) + Cď²* (aq) → Ca?* (aq) + Cd(s) (b) 2B1¯(aq) + Sn²(aq) (c) 2Ag(s) + Ni² (aq) (d) Cu*(aq) + Fe** (aq) Br;(1) + Sn(s) 2Ag(aq) + Ni(s) Cu² (aq) + Fe²* (aq)

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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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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18.16 Predict whether the following reactions would occur
spontaneously in aqueous solution at 25°C. Assume
that the initial concentrations of dissolved species
are all 1.0 M.
Ca* (aq) + Cd(s)
(a) Ca(s) + Cd²+ (aq)
(b) 2Br (aq) + Sn²* (aq) → Br2(1) + Sn(s)
(c) 2Ag(s) + Ni²* (aq)
(d) Cu*(aq) + Fe*(aq)
→ 2Ag" (aq) + Ni(s)
Cu²+ (aq) + Fe2*(aq)

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