Half Equations and the Thermite Process for Welding Railway Tracks

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SUMMARY

The thermite process is a highly effective method for welding railway tracks, utilizing a reaction between aluminum powder and iron(III) oxide. The correct half-equation for the reduction of iron(III) oxide to metallic iron is Fe2O3(s) + 6e- → 2Fe(l) + 3O2-(s). This reaction is part of a redox process that generates molten iron, which fuses the rails together. Understanding the balancing of half-reactions is crucial for accurately representing the chemical processes involved.

PREREQUISITES
  • Knowledge of redox reactions and half-equations
  • Understanding of the thermite process and its applications
  • Familiarity with chemical balancing techniques
  • Basic chemistry concepts, including oxidation states and electron transfer
NEXT STEPS
  • Study the thermite reaction in detail, focusing on the overall chemical equation
  • Learn about redox reactions and how to balance half-equations
  • Explore the applications of the thermite process in industrial welding
  • Investigate the properties and reactions of aluminum powder and iron(III) oxide
USEFUL FOR

Chemistry students, industrial welders, and engineers involved in railway construction and maintenance will benefit from this discussion.

rosie_burk
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The thermite process can be used to weld lengths of railway track together. A mould placed over the ends of the rails to be joined is filled with a charge of aluminium powder and iron(iii) oxide. When the mixture is ignited, a redox reaction occurs to form molten iron, which joins the rails together.

a. Write a half equation for the conversion of iron(iii) oxide to metallic iron.

i got Fe2O3 + 6H+ +6e- = 2Fe + 3H20- but that's wrong according to the book, the answer is Fe2O3(s) + 6e- --> 2Fe(l) + 3O 2- (s). I don't understand why they balanced it using oxygen instead of water.

b. Write the overall equation for the thermite process.
 
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rosie_burk said:
The thermite process can be used to weld lengths of railway track together. A mould placed over the ends of the rails to be joined is filled with a charge of aluminium powder and iron(iii) oxide. When the mixture is ignited, a redox reaction occurs to form molten iron, which joins the rails together.

a. Write a half equation for the conversion of iron(iii) oxide to metallic iron.

i got Fe2O3 + 6H+ +6e- = 2Fe + 3H20- but that's wrong according to the book, the answer is Fe2O3(s) + 6e- --> 2Fe(l) + 3O 2- (s). I don't understand why they balanced it using oxygen instead of water.

Because that would be two half reactions...

6H+ + 3O-2 ------> 3H2O

and

Fe2O3 + 6e- -------------> 2Fe(0) + 3O-2
 

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