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a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to show the conversion of Fe2+ to Fe3+. (iii) Combine the two half equations to give the overall equation.

a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to show the conversion of Fe2+ to Fe3+. (iii) Combine the two half equations to give the overall equation.

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.103QE
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This question is about redox chemistry. a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to show the conversion of Fe2+ to Fe3+. (iii) Combine the two half equations to give the overall equation. b) Using the overall equation from part a, calculate the mass of pure Fe(NH4)2(SO4)2.6H2O which reacts exactly with 25.0 cm³ of 0.0200 mol dm-3 acidified KMNO4. c) Acidified potassium manganate(VII) is an oxidising agent. What is meant by the term oxidising agent? d) The trend in the oxidising ability of the halogens (Group 7) can be seen by carrying out displacement reactions. i. What would you observe when chlorine water is added to a solution of sodium iodide? ii. Write an equation to show the reaction between chlorine iodide. water and sodium iii. State and explain the trend in the oxidising ability down Group 7. The trend in the reducing ability of the halide ions (Group 7) can be seen by adding concentrated sulfuric acid to sodium chloride, sodium bromide and sodium iodide. e) The reaction of sodium bromide and concentrated sulfuric acid produces orange fumes of bromine and sulfur dioxide gas. Write the equation for this reaction. i. Give four observations or names of products when concentrated sulfuric acid reacts with sodium iodide in a redox reaction. ii.
Transcribed Image Text:This question is about redox chemistry. a) (i) Write a half equation to show the conversion of MnO4 toMn2+. (ii) Write a half equation to show the conversion of Fe2+ to Fe3+. (iii) Combine the two half equations to give the overall equation. b) Using the overall equation from part a, calculate the mass of pure Fe(NH4)2(SO4)2.6H2O which reacts exactly with 25.0 cm³ of 0.0200 mol dm-3 acidified KMNO4. c) Acidified potassium manganate(VII) is an oxidising agent. What is meant by the term oxidising agent? d) The trend in the oxidising ability of the halogens (Group 7) can be seen by carrying out displacement reactions. i. What would you observe when chlorine water is added to a solution of sodium iodide? ii. Write an equation to show the reaction between chlorine iodide. water and sodium iii. State and explain the trend in the oxidising ability down Group 7. The trend in the reducing ability of the halide ions (Group 7) can be seen by adding concentrated sulfuric acid to sodium chloride, sodium bromide and sodium iodide. e) The reaction of sodium bromide and concentrated sulfuric acid produces orange fumes of bromine and sulfur dioxide gas. Write the equation for this reaction. i. Give four observations or names of products when concentrated sulfuric acid reacts with sodium iodide in a redox reaction. ii.
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