Redox Example 2 - NO 2 (g) + OH ± (aq) → NO 3 ± + NO 2...

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Lecture Example2: Redox Reaction (basic solution) Balance the following redox reaction: (This reaction is called a disproportionation reaction. One reactant is both oxidized and reduced to produce two different products.) In almost all cases, the oxygen will have a -2 oxidation state in a compound and the hydrogen will have a +1 oxidation state in a compound. Since hydroxide ions are in the original unbalanced equation, we know that the reaction is occurring in basic solution. +4 +5 +3
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Unformatted text preview: NO 2 (g) + OH ± (aq) → NO 3 ± + NO 2 ± + H 2 O Half reactions: +4 +5 NO 2 → NO 3 ± + 1e ± (oxidation, reducing agent) +4 +3 NO 2 + 1e ± → NO 2 ± (reduction, oxidizing agent) Balance the oxygen and hydrogen: (Two hydroxides for every oxygen needed, and one water molecule to balance the other side.) 2 OH ± + NO 2 → NO 3 ± + 1e ± + H 2 O NO 2 + 1e ± → NO 2 ± The charge is already balance; therefore, sum the equations: 2 OH ± + 2 NO 2 → NO 3 ± + NO 2 ± + H 2 O...
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This note was uploaded on 03/17/2010 for the course CH 204 taught by Professor Leytner during the Spring '08 term at University of Texas at Austin.

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