A disproportionate reaction is a redox reaction where the same element is both oxidized and reduced. Let's analyze each option:

1. KMnO₄ → MnSO₄ + Mn₂O₃: Mn is reduced from +7 to +2 and +3. Disproportionation.

2. ${\mathrm{H}}_3{\mathrm{PO}}_3\to {\mathrm{H}}_3{\mathrm{PO}}_4+{\mathrm{PH}}_3$: P is oxidized from +3 to +5 and reduced to -3. Disproportionation.

3. ${\text{PCl}}_{\text{5}}\to {\text{PCl}}_{\text{3}}+{\text{Cl}}_{\text{2}}$: No change in P oxidation state (+5). Not disproportionation.

4. CuCl₂ → Cu₂Cl₂ + Cu: Cu is reduced from +2 to +1 and to 0. Disproportionation.

Final answer: Options 1, 2, and 4 are disproportionate reactions.