Multiply each half reaction to balance e lost and

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Organic Chemistry with Biological Applications
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Chapter 17 / Exercise 17.14
Organic Chemistry with Biological Applications
McMurry
Expert Verified
Multiply each half-reaction to balance e- lost and gained 7.Add and simplify the balanced half-reactions to get the overall reaction. Balance the following half-reactions. 1.Sn2+ + Cr2O72-barb2rightCr3++ Sn4+(acidic) 2.CH3OH + MnO4-barb2rightMn2++ CH2O (acidic) 3.H3AsO4 + Zn barb2rightAsH3+ Zn2+(acidic) Balancing By Half-reaction: Extra Practise 1. Zn(s) + H+(aq) barb2rightZn2++ H2(g) (acidic solution) 2. I-(aq) + NO2-(aq) barb2rightI2(s) + NO (g) (acidic solution) 3. MnO4-(aq) + Cl-(aq) barb2rightMn2+(aq) + Cl2(g) (acidic solution) 4. CrO4-+ S2-barb2rightCr3++ SO42-(acidic solution) 5. H2O2+ NO2-barb2rightH2O + NO3-(acidic solution) 6. IO4-+ I-barb2rightI2(acidic) 7. HgS + Cl-+ NO3-barb2rightHgCl42-+ S + NO (acidic)
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Organic Chemistry with Biological Applications
The document you are viewing contains questions related to this textbook.
Chapter 17 / Exercise 17.14
Organic Chemistry with Biological Applications
McMurry
Expert Verified
15 1.3 Sn2++ Cr2O72-+ 14 H+barb2right2Cr3++ 3Sn4++ 7H22.5 CH3OH + 2 MnO4-+ 6 H+barb2right2 Mn2++ 5 CH2O + 8 H23.H3AsO4 + 4 Zn + 8 H+ barb2rightAsH3+ 4 Zn2++ 4 HBalancing By Half-reaction: Extra Practise 1. Zn(s) + 2 H+(aq) barb2rightZn2++ H2(g) 2. 2 I-(aq) + 2 NO2-(aq) + 4 H+barb2rightI2(s) + 2 NO (g) + 8 H2O 3. 16 H++ 2MnO4-(aq) + 10 Cl-(aq) barb2right2 Mn2+(aq) + 5 Cl2(g) + 2 H24. 2 CrO4-+ S2-+ 8 H+barb2right2 Cr3++ SO42-+ 4 H2O 5. H2O2+ NO2-barb2rightH2O + NO3-6. 2 IO4-+ 14 I-+ 16 H+barb2right8 I2+ 8 H2O7. 3 HgS + 12 Cl-+ 2 NO3-+ 8 H+barb2right3 HgCl42-+ 3 S + 2 NO + 4 H
Answers
O
O
2O
O
2O
16 Chemistry 30 Redox Stoichiometry 1.In a redox titration, 12.50 mL of 0.0800 mol/L K2Cr2O7(aq) was used in an acidic solution to oxidize Sn2+(aq)ions to Sn4+(aq)ions. The volume of K2Cr2O7(aq)used was just sufficient to oxidize all the Sn2+(aq)in 10 mL of the solution. Calculate the concentration of Sn2+(aq)ions in the solution. What color change indicated the endpoint of this titration? (0.30 mol/L) 2.What volume of 0.0500 mol/L KMnO4(aq)is needed to oxidize all the Br-(aq)ions in 25.0 mL of an acidic 0.200 mol/L NaBr(aq)solution. What colour change indicates the endpoint of this reaction?
3.In an experiment, 0.0200 mol/L K2Cr2O7(aq) was used in an acidic solution to oxidize Fe2+(aq)ions to Fe3+(aq)ions. The following data were obtained. Volume of Fe2+(aq)solution (mL)……………..25.0 Final buret reading (K2Cr2O7(aq)) (mL)…….…48.7 Initial buret reading (mL)…….…………………3.7 Calculate the concentration of Fe2+(aq)ions in the solution.
4.The copper (II) ions in a solution can be converted to copper metal by trickling the solution over scrap iron. The reaction produces iron (II) ions from the scrap iron. If the process produces 25.0 L of solution containing 0.00200 mol/L Fe2+(aq)ions, what mass of copper is produced? (3.18 g)

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