Would selenium in the -2 oxidation state be a better reducing agent at pH =3 or

Question

Would selenium in the -2 oxidation state be a better reducing agent at pH =3 or pH=8?

3) 1.2 1.1 HSeC 0.9 0.8 0.7 SeO.2- SeO 0.5 0.4 0.3 HSeo Se 0.1 Seo2 0.1 0.2 0.3 04-H,Se HSe 0.5 0.6 0.7 0.8 0 123 45 6 7 89 10 11 12 13 14 pH a. Would selenium in the-2 oxidation state be a better reducing agent at pH-3 or pH-8? b. Write a balance half-reaction for the conversion of SeOto HSeO under acidic conditions c. At what potential does HSeO, convert Seo, at pH- 4? d. Is Se in the +4 oxidation state a better oxidant at pH 2 or pH 12? e. What does Se in the +4 oxidation state convert to when it is acting as an oxidant at pH- 2? What about when it is acting as a reducing agent at pH- 12? f. What is the slope of the line separating Seo, from HSe? g. What is the slope of the line separating from HSe from Se? h. Why is the line separating Seofrom HSeO, vertical? i. Why are there no horizontal lines in this particular Pourbaix diagram?

Explanation / Answer

The lower the upper boundaries are, the better the reducing agent. So, in the given Pourbouix diagram, the selenium with -2 oxidation act as better reducing agent in basic conditions i.e. pH 8.

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