Question:
Which of the following is not a disproportionation reaction?
Which of the following is not a disproportionation reaction?
Show Hint
To identify disproportionation reactions, track the oxidation number of the same element on both reactant and product sides.
Updated On: Jun 24, 2026
- \(\mathrm{Hg_2Cl_2 \longrightarrow Hg+HgCl_2}\)
- \(\mathrm{4H_3PO_3 \longrightarrow 3H_3PO_4+PH_3}\)
- \(\mathrm{Cl_2+2NaOH \longrightarrow NaCl+NaOCl+H_2O}\)
- \(\mathrm{BaO_2+H_2SO_4 \longrightarrow BaSO_4+H_2O_2}\)
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The Correct Option is D
Solution and Explanation
Step 1: Recall the meaning of disproportionation.
A disproportionation reaction occurs when the same element in a compound gets oxidized and reduced at the same time.
So, we need to check whether the same element shows two different changes in oxidation number.
Step 2: Check option (1).
In \[ \mathrm{Hg_2Cl_2 \longrightarrow Hg+HgCl_2} \] Mercury in \(\mathrm{Hg_2Cl_2}\) has average oxidation state \(+1\).
It changes to \[ 0 \] in \(\mathrm{Hg}\) and \[ +2 \] in \(\mathrm{HgCl_2}\).
So, it is a disproportionation reaction.
Step 3: Check option (2).
In \[ \mathrm{4H_3PO_3 \longrightarrow 3H_3PO_4+PH_3} \] Phosphorus in \(\mathrm{H_3PO_3}\) is \(+3\).
It changes to \(+5\) in \(\mathrm{H_3PO_4}\) and \(-3\) in \(\mathrm{PH_3}\).
So, it is a disproportionation reaction.
Step 4: Check option (3).
In \[ \mathrm{Cl_2+2NaOH \longrightarrow NaCl+NaOCl+H_2O} \] Chlorine changes from \[ 0 \] to \[ -1 \] in \(\mathrm{NaCl}\) and \[ +1 \] in \(\mathrm{NaOCl}\).
So, it is a disproportionation reaction.
Step 5: Check option (4).
In \[ \mathrm{BaO_2+H_2SO_4 \longrightarrow BaSO_4+H_2O_2} \] Oxygen in peroxide remains in the oxidation state \[ -1 \] There is no simultaneous oxidation and reduction of the same element.
Hence, this is not a disproportionation reaction.
Step 6: Final conclusion.
Therefore, the reaction which is not a disproportionation reaction is \[ \boxed{\mathrm{BaO_2+H_2SO_4 \longrightarrow BaSO_4+H_2O_2}} \]
A disproportionation reaction occurs when the same element in a compound gets oxidized and reduced at the same time.
So, we need to check whether the same element shows two different changes in oxidation number.
Step 2: Check option (1).
In \[ \mathrm{Hg_2Cl_2 \longrightarrow Hg+HgCl_2} \] Mercury in \(\mathrm{Hg_2Cl_2}\) has average oxidation state \(+1\).
It changes to \[ 0 \] in \(\mathrm{Hg}\) and \[ +2 \] in \(\mathrm{HgCl_2}\).
So, it is a disproportionation reaction.
Step 3: Check option (2).
In \[ \mathrm{4H_3PO_3 \longrightarrow 3H_3PO_4+PH_3} \] Phosphorus in \(\mathrm{H_3PO_3}\) is \(+3\).
It changes to \(+5\) in \(\mathrm{H_3PO_4}\) and \(-3\) in \(\mathrm{PH_3}\).
So, it is a disproportionation reaction.
Step 4: Check option (3).
In \[ \mathrm{Cl_2+2NaOH \longrightarrow NaCl+NaOCl+H_2O} \] Chlorine changes from \[ 0 \] to \[ -1 \] in \(\mathrm{NaCl}\) and \[ +1 \] in \(\mathrm{NaOCl}\).
So, it is a disproportionation reaction.
Step 5: Check option (4).
In \[ \mathrm{BaO_2+H_2SO_4 \longrightarrow BaSO_4+H_2O_2} \] Oxygen in peroxide remains in the oxidation state \[ -1 \] There is no simultaneous oxidation and reduction of the same element.
Hence, this is not a disproportionation reaction.
Step 6: Final conclusion.
Therefore, the reaction which is not a disproportionation reaction is \[ \boxed{\mathrm{BaO_2+H_2SO_4 \longrightarrow BaSO_4+H_2O_2}} \]
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