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12 Dec 2019

Consider the hydrolysis of pure water (an electrolytic cell):

Anode: 2 H2O(l ) ? O2(g ) + 4 H+(aq ) + 4 e? E° = ?1.23 V

Cathode: 2 H2O(l ) + 2 e? ? H2(g ) + 2 OH?(aq ) E° = ?0.83 V

This system:

Can do work as the reaction proceeds
Must have work done on it in order to proceed
Cannot ever react

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Trinidad Tremblay
Trinidad TremblayLv2
13 Dec 2019

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Related questions

1) A constant current of 0.800 A is run through the electrolytic cell in order to produce oxygen (gas) at the anode:

2 H2O → O2(g) + 4 e- + 4 H+

The amount (in grams) of O2 obtained after 15.2 min of electrolysis is [X] g

2) Electrolysis of a solution of Tl3+ produces deposition of elemental thallium, Tl, at the cathode. The time (in min.) needed for a constant current of 1.20 A to deposit 0.500 g of Tl(s) is [X] min.

3) An electrochemical cell is described by the following line notation:

Zn(s) ǀ Zn2+(aq) (0.0420 M) ǀǀ Tl3+(aq) (9.06×10-2 M), Tl+(aq) (0.0400 M) ǀ Pt(s).

Given: E°(Zn2+/Zn) = - 0.763 V; E°(Tl3+/Tl+) = + 1.25 V.

The potential on the cathode half-cell, E+ = V; the potential on the anode half-cell, E- = V; and the overall cell potential, Ecell = V.

4) Consider electrolysis of molten copper bromide, CuBr2. What is the product of this process obtained (a) at the cathode? (b) at the anode?

1. a) Cathode: Cu(s);
(b) Anode: Br2(l)

2. (a) Cathode: Br2(l);

(b) Anode: Cu(s)

3. (a) Cathode: Cu2+;

(b) Anode: Br-

4. (a) Cathode: Br-;

(b) Anode: Cu2+

5. (a) Cathode: Cu(s);

(b) Anode: O2(g)

6. (a) Cathode: H2(g);

(b) Anode: Cu2+


Show transcribed image text

3) The voltaic cell described by the cell notation has an Eo of 0.68 V. Calculate the Wmax (kJ) the cell has done if 6.4700 mol of MnO4-(aq) (Molar Mass - 118.94 g/mol) reacts. Round your answer to 3 significant figures.

Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)

St. Red. Pot. (V)

VO2+/VO2+: +1.00

MnO4-/MnO2 :+1.68

Faraday's Constant

F = 96485 C

4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures.

Pt(s), H2(g) l H2O(l), OH-(aq) ll O2(g) l OH-(aq) l Pt(s)

St. Red. Pot. (V)

H2O/H2: -0.83

O2/OH- : +0.40

Faraday's Constant

F = 96485 C

5) The electrochemical cell described by the balanced chemical equation has a standard cell potential of -0.37 V. Calculate the value (kJ) for the standard free energy change of the cell. Round your answer to 3 significant figures.

Sn4+(aq) + 2Cu(s) → Sn2+(aq) + 2Cu+(aq)

St. Red. Pot. (V)

Cu+/Cu: +0.52

Sn4+/Sn2+: +0.15

Faraday's Constant

F = 96485 C

6)The electrochemical cell described by the cell notation has an Eocell of 4.05 V. Calculate the maximum electrical work (kJ) the cell has done if 375.44 g of F2(g) (Molar Mass - 38.00 g/mol) reacts. Round your answer to 3 significant figures.

Mn(s) l Mn2+(aq) ll F2(g) l F-(aq) l Pt(s)

St. Red. Pot. (V)

Mn2+/Mn: -1.18

F2/F- : +2.87

Faraday's Constant

F = 96485 C

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