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From the given reactions identify the disproportionation reaction i) Cl 2 ( g ) + 2 KI ( aq ) ⟶ 2 KCl ( aq ) + I 2 ( s ) ii) Cl 2 ( g ) + 2 OH - ( aq ) ⟶ ClO - ( aq ) + Cl - ( aq ) + H 2 O ( l ) iii) Mg ( s ) + 2 HCl ( aq ) ⟶ MgCl 2 ( aq ) + H 2 ( g ) iv) 2 H 2 O 2 ( aq ) ⟶ 2 H 2 O ( l ) + O 2 ( g )

Options

  1. A(i) and (iv)
  2. B(ii) and (iv)
  3. C(ii) and (iii)
  4. D(i) and (ii)

Correct answer

B. (ii) and (iv)

Step-by-step solution

The reaction in which one reactant gets oxidized, and the same reactant gets reduced is known as disproportionation reaction. Cl 0 2 ( g ) + 2 K I - 1 ( aq ) ⟶ 2 K C 0 l ( aq ) + I - 1 2 ( s ) In the above reaction different elements undergoing oxidation and reduction. Hence, It is not a disproportionation reaction. Cl 0 2 ( g ) + 2 OH - ( aq ) ⟶ Cl + 1 O - ( aq ) + Cl - ( aq ) + H 2 O ( l ) In the above reaction chlorine is undergoing oxidation as well as reduction. Hence, It is a disproportionation

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