standard electrode potential

2010-11-29 7:33 am

What are the standard electrode potential and half equations of the following?
H2O (g) --> H2 (g) (For this case, oxide rather than hydroxide is formed)
nitrate ion (aq) --> NO (g)
SO2 (g) --> S (s)
O2 (g) --> oxide (s)
sulphite ion (aq) --> sulphate ion (aq)
S (s) --> SO2 (g)
NO (g) --> NO2 (g)
NH3 (g) --> N2 (g)

What are the two half equations that make up this overall redox reaction?
What are the standard electrode potential of those half equations?
P4 (s) + 10Cl2 (g) --> 4PCl5 (s)
C (s) + O2 (g)--> CO2 (g)
C (s) + PbO (s) --> C0 (g) + Pb (s)

回答 (1)

己式庚辛

2010-12-02 10:02 pm

✔ 最佳答案

1.
Standard reduction potential requires species at Standard conditions. your water is in gas state ---- not Standard!

2.
NO3(-) + 4H(+) + 3e- ------> NO + 2H2O
E = +0.96V

3.
SO2 + 4H(+) + 4e- ------> S + 2H2O
E = +0.50V

4.
oxide cannot exist in aqueous solutions...

5.
SO3(2-) + 2OH(-) ------> SO4(2-) + H2O + 2e-
E = +0.93V

6, 7.
cannot find at this moment.

8, 9, 10:
ions are not involved in these reactions; there're mainly formation and cleavage of covalent bonds. thus they don't have half-equations nor electrode potentials.

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