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General Chemistry II-Lecture,Section-1-Spring 2025

General Chemistry II-Lecture,Section-1-Spring 2025

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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment).

The standard reduction potentials are as follows:

MnO₄^- + 8H⁺ + 5e^- ® Mn²⁺ + 4H₂O	E° = 1.51 V
Cr₂O₇^2- +14H⁺ + 6e^- ® 2 Cr³⁺ +7H₂O	E° = 1.33 V

What is the value of

Q, the reaction quotient, for this cell reaction?

6.7 ´ 10⁴⁰

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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment).

The standard reduction potentials are as follows:

MnO₄^- + 8H⁺ + 5e^- ® Mn²⁺ + 4H₂O	E° = 1.51 V
Cr₂O₇^2- +14H⁺ + 6e^- ® 2Cr³⁺ +7H₂O	E° = 1.33 V

In the balanced cell reaction, what is the stoichiometric coefficient for H

⁺?

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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment).

The standard reduction potentials are as follows:

MnO₄^- + 8H⁺ + 5e^- ® Mn²⁺ + 4H₂O	E° = 1.51 V
Cr₂O₇^2- +14H⁺ + 6e^- ® 2 Cr³⁺ +7H₂O	E° = 1.33 V

How many electrons are transferred in the balanced reaction (that is, what will be the value of

n in the Nernst equation)?

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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment).

The standard reduction potentials are as follows:

MnO₄^- + 8H⁺ + 5e^- ® Mn²⁺ + 4H₂O	E° = 1.51 V
Cr₂O₇^2- +14H⁺ + 6e^- ® 2 Cr³⁺ +7H₂O	E° = 1.33 V

What is the value of the equilibrium constant at 25°C for the net spontaneous cell reaction?

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Gold (atomic mass = 197 g/mol) is plated from a solution of chlorauric acid, HAuCl₄; it deposits on the cathode. Calculate the time it takes to deposit 0.65 g of gold, passing a current of 0.14 amperes. (1 faraday = 96,485 coulombs)

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The following two half-reactions take place in a galvanic cell. At standard conditions, what species are produced at each electrode?

Sn²⁺ + 2e^- ® Sn		E° = -0.14 V
Cu²⁺ + 2e^- ® Cu		E° = 0.34 V

Sn is produced at the cathode, and Cu²⁺ is produced at the anode.

Sn is produced at the anode, and Cu²⁺ is produced at the cathode.

Cu is produced at the anode, and Sn²⁺ is produced at the cathode.

Cu is produced at the cathode, and Sn²⁺ is produced at the anode.

Sn is produced at the anode, and Cu is produced at the cathode.

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The following questions refer to a galvanic cell that utilizes the following reaction (unbalanced):

(AuCl₄)^-(aq) + Cu(s) ® Au(s) + Cl^-(aq)+ Cu²⁺(aq)

Determine the number of electrons transferred during the reaction (when balanced).

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The standard free energies of formation of several aqueous species are

		kJ/mol
H⁺(aq)	0
H₂O(l)	-237
CH₃OH(aq)	-163
HCOOH(aq)	-351
e^-	0

What is the standard reduction potential of methanoic acid in aqueous solution (that is, for HCOOH + 4H⁺ + 4e^- ® CH₃OH + H₂O)?

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What quantity of charge is required to reduce 31.2 g of CrCl₃ to chromium metal? (1 faraday = 96,485 coulombs)

3.80 ´ 10⁴ C

7.60 ´ 10⁴ C

1.74 ´ 10⁵ C

1.90 ´ 10⁴ C

5.70 ´ 10⁴ C

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An excess of finely divided iron is stirred up with a solution that contains Cu²⁺ ion, and the system is allowed to come to equilibrium. The solid materials are then filtered off, and electrodes of solid copper and solid iron are inserted into the remaining solution. What is the value of the ratio [Fe²⁺]/[Cu²⁺] at 25°C?

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