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11 Dec 2019

1. Balance the following reactions and assign oxidation numbers for each of the elements participating. Assume that reaction b) occurs in basic conditions. a. NO(g) + O2(g) ＝NO2(g) b. Mn3+ ＝ MnO2 + Mn2+

2. a) Write the Nernst equation for: O2(g) + 4H+ (aq) + 4e- ＝2H2O(l) b) What is the potential for the reduction of O2 at pH = 7 and p(O2) = 0.20 bar?

3.Use the Latimer diagram for chlorine to determine the potential for reduction of ClO4 - to Cl2. Write a balanced equation for this half reaction.

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Related questions

Complete and balanced the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction.

  1. (Sn2+(aq) → Sn4+(aq) (acidic solution) ,

  2. TiO2(s) → Ti2+(aq), (acidic solution)

  3. ClO3-(aq) → Cl-(aq) , (acidic solution)

  4. N2→ 2NH4+(aq), (acidic solution)

  5. 4OH- (aq) → O2 (g) , (basic solution)

  6. SO32- (aq) → SO42-(aq), (basic solution)

  7. N2(g) →NH3(g), (basic solution)

One Class Solution:-

  1. Sn2+(aq) → Sn4+(aq) +2e-,

  2. TiO2(s) +2e-+ 4H+→ Ti2+ + 2H2O,

  3. ClO3-+ 6H+ + 6e-→ Cl- + 3H2O,

  4. N2+6e-+ 8H+ → 2NH4+,

  5. 4OH- → O2 +2H2O+4e-,

  6. SO32- + 2OH- → SO42-+2e- + H2O,

  7. N2(g) + 6H2O+ 6e- →2NH3(g) + 6OH-(aq),

a) oxidation, b) reduction, c) reduction, d) reduction, e) oxidation, f) oxidation, g) reduction

1. Write the two step sequence and net reaction for the reaction of nitric acid with CH3CH2NH2.

2. Write a balanced equation for the following reactions , identifying the reduction and oxidation half reactions, plus oxidizing and reducing reagents.

a. Conducted in a Basic solution: K(s) + H2O K+(aq) + H2 (g)

b. COndicted in an Acidic solution: O2(g) + Br-(aq) H2O + Br2

The following diagram, called a Latimer diagram, summarizes the standard reduction potentials for various nitrogen-containing compounds and ions in acidic aqueous solution. It contains useful data for this HW set.

An arrow represents the “properly balanced reduction half-reaction” between the oxidized species on the left and the reduced species on the right of the arrow. The potential value over each arrow is the standard reduction potential E 0 red for that properly balanced half-reaction. For example, from this diagram, you can write NO3 – (aq) + e– + 2 H+ (aq)  NO2(g) + H2O(l); E 0 red = +0.79 V

(2) (16 pts) Use the Latimer diagram above for this question.

(a) (6 pts) NO2(g) disproportionates spontaneously into nitric acid and nitrous acid in acidic media. Show this by writing the balanced chemical reaction and evaluating the standard emf for the reaction.

(b) (6 pts) Nitrous acid will not disproportionate spontaneously to nitrogen dioxide and nitric oxide. Show this by writing the balanced chemical reaction and evaluating the standard emf for the reaction.

(c) (4 pts) Given that the definition of 1 volt = 1 joule/coulomb, show that the reduction of the nitrate ion to nitrogen gas in acidic media has a standard reduction potential of +1.25 V.

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