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Which of the following equations represent redox reactions and what are the values for ‘p’ and ‘q’ in these equations?

  • Equation 1 : Fe2O3(s)+2Al(s)⟶Al2O3(s)+pFe(l)+Heat\text{Fe}2 \text O3 (\text s) + 2\text {Al}(\text s) \longrightarrow \text{Al}2 \text O3 (\text s) + \text {pFe}(\text l) + \text {Heat}
  • Equation 2 : 2C4H10(g)+13O2(g)→Δ8CO2(g)+qH2O(g)2\text C4 \text H{10} (\text g) + 13\text O2(\text g) \xrightarrow {\Delta} 8\text {CO}2 (\text g) + \text {qH}_2 \text O(\text g)

options

  1. Only equation 1 is a redox reaction, p = 1 and q = 3
  2. Both equations 1 and 2 are redox reactions, p = 2 and q = 4
  3. Only equation 2 is a redox reaction, p = 2 and q = 10
  4. Both equations 1 and 2 are redox reactions, p = 2 and q = 10

Chemical Reaction

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Answer

Both equations 1 and 2 are redox reactions, p = 2 and q = 10

Reason —

  • Equation 1 is a thermit reaction in which Al is oxidized to Al2O3 and Fe2O3 is reduced to Fe thus it is a redox reaction which is given by:
    Fe2O3(s)+2Al(s)⟶Al2O3(s)+2Fe(l)+Heat\text{Fe}2 \text O3 (\text s) + 2\text {Al}(\text s) \longrightarrow \text{Al}2 \text O3 (\text s) + 2\text {Fe}(\text l) + \text {Heat}
    So, here, p = 2

  • Equation 2 is reaction of combustion of butane in which carbon and hydrogen are oxidized but oxygen is reduced to O in CO2/H2O thus it is a redox process which is given by:
    2C4H10(g)+13O2(s)→Δ8CO2(g)+10H2O(g)2\text C4 \text H{10} (\text g) + 13\text O2(\text s) \xrightarrow {\Delta} 8\text {CO}2 (\text g) + 10\text H_2 \text O(\text g)
    So, here, q = 10

Hence, both equations 1 and 2 are redox reactions, p = 2 and q = 10.

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