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Which of the following chemical reaction...

Which of the following chemical reactions depicts the oxidizing behaviour of `H_(2)SO_(4)` ?

A

`2HI+H_(2)SO_(4)toI_(2)+SO_(2)+2H_(2)O`

B

`Ca(OH)_(2)+H_(2)SO_(4)to CaSO_(4)+2H_(2)O`

C

`NaCI+H_(2)SO_(4)to NaHSO_(4)+HCI`

D

`2PCI_(5)+H_(2)SO_(4)to 2POCI_(3)+2HCI+SO_(2)CI_(2)`

Text Solution

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The correct Answer is:
To determine which of the given reactions depicts the oxidizing behavior of sulfuric acid (H₂SO₄), we need to analyze each reaction for oxidation and reduction processes. An oxidizing agent is a substance that gains electrons (is reduced) while causing another substance to lose electrons (is oxidized). ### Step-by-Step Solution: 1. **Identify the Reactions**: We have four reactions to analyze: - **Option A**: HI + H₂SO₄ → I₂ + SO₂ + 2H₂O - **Option B**: Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2H₂O - **Option C**: NaCl + H₂SO₄ → NaHSO₄ + HCl - **Option D**: PCl₅ + H₂SO₄ → POCl₃ + HCl + SOCl₂ 2. **Analyze Option A**: - **Reactants**: HI (oxidation state of I is -1) and H₂SO₄ (oxidation state of S is +6). - **Products**: I₂ (oxidation state of I is 0) and SO₂ (oxidation state of S is +4). - **Oxidation State Change**: - Iodine: -1 to 0 (oxidation, loss of electrons) - Sulfur: +6 to +4 (reduction, gain of electrons) - **Conclusion**: This is a redox reaction where H₂SO₄ acts as an oxidizing agent. 3. **Analyze Option B**: - **Reactants**: Ca(OH)₂ (Ca is +2, O is -2, H is +1) and H₂SO₄ (S is +6). - **Products**: CaSO₄ (Ca is +2, S is +6, O is -2) and H₂O (H is +1, O is -2). - **Oxidation State Change**: No change in oxidation states. - **Conclusion**: This is not a redox reaction. 4. **Analyze Option C**: - **Reactants**: NaCl (Na is +1, Cl is -1) and H₂SO₄ (S is +6). - **Products**: NaHSO₄ (Na is +1, S is +6) and HCl (H is +1, Cl is -1). - **Oxidation State Change**: No change in oxidation states. - **Conclusion**: This is not a redox reaction. 5. **Analyze Option D**: - **Reactants**: PCl₅ (P is +5, Cl is -1) and H₂SO₄ (S is +6). - **Products**: POCl₃ (P is +5, Cl is -1) and HCl (H is +1, Cl is -1) and SOCl₂ (S is +6, Cl is -1). - **Oxidation State Change**: No change in oxidation states. - **Conclusion**: This is not a redox reaction. ### Final Conclusion: The only reaction that depicts the oxidizing behavior of H₂SO₄ is **Option A**: HI + H₂SO₄ → I₂ + SO₂ + 2H₂O.
To determine which of the given reactions depicts the oxidizing behavior of sulfuric acid (H₂SO₄), we need to analyze each reaction for oxidation and reduction processes. An oxidizing agent is a substance that gains electrons (is reduced) while causing another substance to lose electrons (is oxidized). ### Step-by-Step Solution: 1. **Identify the Reactions**: We have four reactions to analyze: - **Option A**: HI + H₂SO₄ → I₂ + SO₂ + 2H₂O - **Option B**: Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2H₂O ...
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Knowledge Check

  • Which of the following equations depict the oxidising nature of H_(2)O_(2) ?

    A
    `2MnO_(4)^(-)+6H^(+)+5H_(2)O_(2)rarr 2Mn^(2+)+8H_(2)O+5O_(2)`
    B
    `2Fe^(3+)+2H^(+)+H_(2)O_(2)rarr 2Fe^(2+)+2H_(2)O+O_(2)`
    C
    `2I^(-)+2H^(+)+H_(2)O_(2)rarr I_(2)+2H_(2)O`
    D
    `KIO_(4)+H_(2)O_(2)rarr KIO_(3)+H_(2)O+O_(2)`

  • Which of the following equation depicts reducing nature of H_(2)O_(2) ?

    A
    `PbS + 4H_(2)O_(2) to PbSO_(4) + 4H_(2)O`
    B
    `Ag_(2)O + H_(2)O_(2) to 2Ag + H_(2)O + O_(2)`
    C
    `2HCHO + H_(2)O_(2) to 2HCOOH + H_(2)O`
    D
    `Na_(2)SO_(3) + H_(2)O_(2) to Na_(2)SO_(4) + H_(2)O`

  • Which of the following equation depicts reducing nature of H_(2)O_(2) ?

    A
    `2[Fe(CN)_(6)]^(4-)+2H^(+)+H_(2)O_(2)rarr2[Fe(CN)_(6)]^(3-)+2H_(2)O`
    B
    `I_(2)+H_(2)O_(2)+2OH^(-)rarr 2I^(-)+2H_(2)O+O_(2)`
    C
    `Mn^(2+)+H_(2)O_(2)rarr Mn^(4+)+2OH^(-)`
    D
    `PbS+4H_(2)O_(2)rarr PbSO_(4)+4H_(2)O`

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    H_(2)SO_(4) acts as an oxidising agent, a dehydrating agent, and an acid. Among each of the following reactions, which behaviour is shown by H_(2)SO_(4) ? a. C_(6)H_(12)O_(6)+H_(2)SO_(4)(conc)rarr6C+6H_(2)O b. 5H_(2)SO_(4)(conc)+4ZnrarrH_(2)S+4Zn^(2+)+4SO_(4)^(2-)+4H_(2)O c. H_(2)SO_(4)(dil)+ZnrarrZn^(2+)+H_(2)+SO_(4)^(2-) d. H_(2)SO_(4)(dil)ZnCO_(3)rarrZn^(2+)+CO_(2)+CO_(2)+SO_(4)^(2-)+H_(2)O

    Which of the following equation depicts reducing nature of H_(2)O_(2) ?

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