Using the values from the table of standard reduction potentials, calculate the cell potentials ofthe following cells:(a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s)(b) Zn(s) | Zn²-(aq) | Cr**(aq) | Cr(s)(c) Fe(s), FeS(3) | S² (aq) | Sn²*(aq) | Sn(s)Calculate the standard free energy change of the following reactions using the standard cellpotentials for the half reactions that are involved:(a) Fe(s) + Hg;*"(aq) →F²²*(aq) + 2 Hg(4)(b) Fe*"(aq) + Ag(s) + CI (aq) → Fe²"(aq) + AgC(s)Use the Nernst equation to calculate the cell potential of the given cell at 298K:12 Ag"(aq)(0.50 M) + Ni(s) → 2 Ag(s) + Ni²^(aq)(0.20 M)Write the equilibrium expressions for each of the following reactions:(a) CaCO,(s) 2C2²*(aq) + CO,²-(aq)(b) Mg;(PO4);(s) 23 Mg²*(aq) + 2 PO,"(aq)(c) CO(g) + NO;(g)=C0;(g) + NO(g)Which of the following is more likely to precipitate the sulfate ion?(a) PbSO4(9) Pb²*(aq) + SO,²"(aq) K= 1.8 × 10(b) CASO,(s) #Ca²*(aq) + SO,²-(aq) K=9.1 × 10-6

Ga/Ga+3∥Ag+/AgE0Ga+3/Ga=-0.56 V (anode)E0Ag+/Ag=+0.80 V (cathode)E0cell =E0c-E0A=0.80-(-0.56) =+1.36…

Using the values from the table of standard reduction potentials, calculate the cell potentials of the following cells: (a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s) (b) Zn(s) | Zn²“(aq) | Cr*(aq) | Cr(s) (c) Fe(s), FeS(s) | S²-(aq) || Sn²*(aq) | Sn(s)

Using the values from the table of standard reduction potentials, calculate the cell potentials of the following cells: (a) Ga(s) | Ga³"(aq) || Ag(aq) | Ag(s) (b) Zn(s) | Zn²“(aq) | Cr(aq) | Cr(s) (c) Fe(s), FeS(s) | S²-(aq) || Sn²*(aq) | Sn(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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Concept explainers

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.

Question

Using the values from the table of standard reduction potentials, calculate the cell potentials of
the following cells:
(a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s)
(b) Zn(s) | Zn²-(aq) | Cr**(aq) | Cr(s)
(c) Fe(s), FeS(3) | S² (aq) | Sn²*(aq) | Sn(s)
Calculate the standard free energy change of the following reactions using the standard cell
potentials for the half reactions that are involved:
(a) Fe(s) + Hg;*"(aq) →F²²*(aq) + 2 Hg(4)
(b) Fe*"(aq) + Ag(s) + CI (aq) → Fe²"(aq) + AgC(s)
Use the Nernst equation to calculate the cell potential of the given cell at 298K:
12 Ag"(aq)(0.50 M) + Ni(s) → 2 Ag(s) + Ni²^(aq)(0.20 M)
Write the equilibrium expressions for each of the following reactions:
(a) CaCO,(s) 2C2²*(aq) + CO,²-(aq)
(b) Mg;(PO4);(s) 23 Mg²*(aq) + 2 PO,"(aq)
(c) CO(g) + NO;(g)=C0;(g) + NO(g)
Which of the following is more likely to precipitate the sulfate ion?
(a) PbSO4(9) Pb²*(aq) + SO,²"(aq) K= 1.8 × 10
(b) CASO,(s) #Ca²*(aq) + SO,²-(aq) K=9.1 × 10-6

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