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1. Write a balanced equation for the oxidation of phosphorus by nitric acid, which is described by Pa(s) + H(aq) + NO₂ (aq)H₂PO4 (aq) + NO(g)

1. Write a balanced equation for the oxidation of phosphorus by nitric acid, which is described by Pa(s) + H(aq) + NO₂ (aq)H₂PO4 (aq) + NO(g)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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1. Write a balanced equation for the oxidation of phosphorus by nitric acid, which is described by Pa(s) + H(aq) + NO3(aq)H₂PO4 (aq) + NO(g) 2. Cyanate ion in waste solutions from gold-mining operations can be destroyed by treatment with hypochlorite ion in basic solution. Write a balanced oxidation-reduction equation for this reaction. OCN (aq) + OCT (aq) + OH(aq) CO₂ (aq) + N₂(g) + Cr(aq) + H₂O(1) (Hint: Notice that in the oxidation half-reaction, OCN yields two products.) 3. In basic solution, Br₂ disproportionates to bromide ions and bromate ions. Use the half- reaction method to balance the equation for this reaction: Br₂(1) Br(aq) + BrO₂ (aq) 4. Permanganate ion, MnO4, is used in the laboratory as an oxidizing agent; thiosulfate ion, S₂0₂², is used as a reducing agent. Write a balanced equation for the reaction of these ions in an acidic aqueous solution to produce manganese(II) ion and sulfate ion.
Transcribed Image Text:1. Write a balanced equation for the oxidation of phosphorus by nitric acid, which is described by Pa(s) + H(aq) + NO3(aq)H₂PO4 (aq) + NO(g) 2. Cyanate ion in waste solutions from gold-mining operations can be destroyed by treatment with hypochlorite ion in basic solution. Write a balanced oxidation-reduction equation for this reaction. OCN (aq) + OCT (aq) + OH(aq) CO₂ (aq) + N₂(g) + Cr(aq) + H₂O(1) (Hint: Notice that in the oxidation half-reaction, OCN yields two products.) 3. In basic solution, Br₂ disproportionates to bromide ions and bromate ions. Use the half- reaction method to balance the equation for this reaction: Br₂(1) Br(aq) + BrO₂ (aq) 4. Permanganate ion, MnO4, is used in the laboratory as an oxidizing agent; thiosulfate ion, S₂0₂², is used as a reducing agent. Write a balanced equation for the reaction of these ions in an acidic aqueous solution to produce manganese(II) ion and sulfate ion.
Balancing Oxidation-Reduction Reactions using Method of Half Reactions Reactions Occur in acid 1. Assign oxidation numbers to determine what is oxidized and what is reduced. 2. Write the oxidation and reduction half-reactions. 3. Balance each half-reaction. 1. Balance elements other than H and O. 2. Balance O by adding H₂O. 3. Balance H by adding H". 4. Balance charge by adding electrons 4. Multiply the half-reactions by integers so that the electrons gained and lost are the same. 5. Add the half-reactions, subtracting things that appear on both sides. 6. Make sure the equation is balanced according to mass. 7. Make sure the equation is balanced according to charge. Reaction Occurs in Base 8. If a reaction occurs in a basic solution, one can balance it as if it occurred. in acid. 9. Once the equation is balanced, add OH to each side to "neutralize" the H' in the equation an create water in its place. 10. If this produces water on both sides, you might have to subtract water from each side.
Transcribed Image Text:Balancing Oxidation-Reduction Reactions using Method of Half Reactions Reactions Occur in acid 1. Assign oxidation numbers to determine what is oxidized and what is reduced. 2. Write the oxidation and reduction half-reactions. 3. Balance each half-reaction. 1. Balance elements other than H and O. 2. Balance O by adding H₂O. 3. Balance H by adding H". 4. Balance charge by adding electrons 4. Multiply the half-reactions by integers so that the electrons gained and lost are the same. 5. Add the half-reactions, subtracting things that appear on both sides. 6. Make sure the equation is balanced according to mass. 7. Make sure the equation is balanced according to charge. Reaction Occurs in Base 8. If a reaction occurs in a basic solution, one can balance it as if it occurred. in acid. 9. Once the equation is balanced, add OH to each side to "neutralize" the H' in the equation an create water in its place. 10. If this produces water on both sides, you might have to subtract water from each side.
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